What are the two general concepts involved in equilibrium?

Consider the following generic equilibrium in which a solid reactant is in equilibrium with a gaseous product: \(A(s) \rightleftharpoons B(g)\) These diagrams represent the reaction mixture at the following points: (a) initially; (b) after a short period of time has passed; and (c) at equilibrium. For each diagram, calculate the concentrations of the spheres representing A(s) and B(g). Assume that each block in the grid has an area of 1 cm2 and report your answer in units of spheres/cm2. (Since the spheres in the solid are not free to move, the solid only occupies the area that it covers. The spheres in the solid, however, are free to move and therefore occupy the entire grid.) What do you notice about the concentrations of A(s) and B(g) in these representations? Write an equilibrium expression for the generic reaction and use the results of your calculations to explain why A(s) is not included in the expression. Equation Transcription: ? Text Transcription: A(s)? B(g)

What is a fuel-cell electric vehicle?

What is an oxidation-reduction or redox reaction?

What is organic chemistry?

How do most chemical reactions occur?

What normally happens to the rate of the forward reaction as a reaction proceeds?

Explain how dynamic chemical equilibrium involves the concepts of sameness and constancy.

What factors influence reaction rates? How?

What is dynamic chemical equilibrium?

Explain why the concentrations of reactants and products are not necessarily the same at equilibrium.

What is the equilibrium constant? Why is it significant?

Write the expression for the equilibrium constant for the following generic chemical equation. \(a \mathrm{~A}+b \mathrm{~B} \rightleftharpoons c \mathrm{C}+d \mathrm{D}\) Equation Transcription: ? Text Transcription: ????A + ????B ? ????C + ????D

Devise your own analogy—like the Narnia and Middle Earth analogy in the chapter—to explain chemical equilibrium.

What does a small equilibrium constant tell you about a reaction? A large equilibrium constant?

Why are solids and liquids omitted from the equilibrium expression?

Will the concentrations of reactants and products always be the same in every equilibrium mixture of a particular reaction at a given temperature? Explain.

Apply Le Châtelier’s principle to your analogy from Question 12. Question 12: Write the expression for the equilibrium constant for the following generic chemical equation. \(a \mathrm{A}+b \mathrm{B} \rightleftharpoons c \mathrm{C}+d \mathrm{D}\) Equation Transcription: ? Text Transcription: aA+bB rightleft harpoons cC+dD

What is Le Châtelier’s principle?

What is the effect of increasing the concentration of a reactant in a reaction mixture at equilibrium?

What is the effect of decreasing the concentration of a reactant in a reaction mixture at equilibrium?

What is the effect of increasing the concentration of a product in a reaction mixture at equilibrium?

What is the effect of decreasing the concentration of a product in a reaction mixture at equilibrium?

What is the effect of increasing the pressure of a reaction mixture at equilibrium if the reactant side has fewer moles of gas particles than the product side?

What is the effect of increasing the pressure of a reaction mixture at equilibrium if the product side has fewer moles of gas particles than the reactant side?

What is the effect of decreasing the pressure of a reaction mixture at equilibrium if the reactant side has fewer moles of gas particles than the product side?

What is the effect of decreasing the pressure of a reaction mixture at equilibrium if the product side has fewer moles of gas particles than the reactant side?

What is the effect of increasing the temperature of an endothermic reaction mixture at equilibrium? Of decreasing the temperature?

What is the effect of increasing the temperature of an exothermic reaction mixture at equilibrium? Of decreasing the temperature?

What is the solubility-product constant? What does it signify?

What are solubility and molar solubility?

Write an expression for the solubility-product constant of \(AB_2(s)\). Assume that an ion of B has a charge of 1- (that is, \(B^-\)). Equation Transcription: Text Transcription: AB_2(s) B^-

Write an expression for the solubility-product constant of \(A_2B(s)\). Assume that an ion of B has a charge of 2- (that is, \(B^{2-}\)). Equation Transcription: Text Transcription: A_2B(s) B^{2-}

What is activation energy for a chemical reaction?

Explain why two reactants with a large \(K_{\mathrm {eq}}\) for a particular reaction might not react immediately when combined. Equation Transcription: Text Transcription: K_eq

What is the effect of a catalyst on a reaction? Why are catalysts so important to chemistry?

Does a catalyst affect the value of the equilibrium constant?

What are enzymes?

Two gaseous reactants are allowed to react in a 1-L flask, and the reaction rate is measured. The experiment is repeated with the same amount of each reactant and at the same temperature in a 2-L flask (so the concentration of each reactant is less). What is likely to happen to the measured reaction rate in the second experiment compared to the first?

The rate of phosphorus pentachloride decomposition is measured at a \(\mathrm {PCl_5}\) pressure of 0.015 atm and then again at a \(\mathrm {PCl_5}\) pressure of 0.30 atm. The temperature is identical in both measurements. Which rate is likely to be faster? Equation Transcription: Text Transcription: PCl_5

The body temperature of cold-blooded animals varies with the ambient temperature. From the point of view of reaction rates, explain why cold-blooded animals are more sluggish at cold temperatures.

The rate of a particular reaction doubles when the temperature increases from \(\mathrm {25~ ^\circ C}\) to \(\mathrm {35~ ^\circ C}\). Explain why this happens. Equation Transcription: Text Transcription: 25 ^oC 35 ^oC

The initial rate of a chemical reaction was measured, and one of the reactants was found to be reacting at a rate of 0.0011 mol/L s. The reaction was allowed to proceed for 15 minutes, and the rate was measured again. What would you predict about the second measured rate relative to the first?

When vinegar is added to a solution of sodium bicarbonate, the mixture immediately begins to bubble furiously. As time passes, however, there is less and less bubbling. Explain why this happen

Write an equilibrium expression for each chemical equation. (a) \(2 \mathrm{NO}_{2}(g) \rightleftharpoons \mathrm{N}_{2} \mathrm{O}_{4}(g)\) (b) \(2 B r N O(g) \rightleftharpoons 2 N O(g)+B r_{2}(g)\) (c) \(\mathrm{H}_{2} \mathrm{O}(\mathrm{g})+\mathrm{CO}(\mathrm{g}) \rightleftharpoons \mathrm{H}_{2}(\mathrm{~g})+\mathrm{CO}_{2}(\mathrm{~g})\) (d) \(\mathrm{CH}_{4}(g)+2 \mathrm{H}_{2} \mathrm{~S}(g) \rightleftharpoons \mathrm{CS}_{2}(g)+4 \mathrm{H}_{2}(g)\) Equation Transcription: ? ? ? ? Text Transcription: 2 NO_2(g) ? N_2O_4(g) 2 BrNO(g) ? 2 NO(g) + Br_2(g) H_2O(g) + CO(g) ? H_2(g)+CO_2(g) CH_4(g)+2H_2S(g) ? CS_2(g)+4 H_2(g)

Write an equilibrium expression for each chemical equation. (a) \(2 \mathrm{CO}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{CO}_{2}(g)\) (b) \(\mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{NO}(g)\) (c) \(\mathrm{SbCl}_{5}(g) \rightleftharpoons \mathrm{SbCl}_{3}(g)+\mathrm{Cl}_{2}(g)\) (d) \(\mathrm{CO}(g)+\mathrm{Cl}_{2}(g) \rightleftharpoons \mathrm{COCl}_{2}(g)\)

Write an equilibrium expression for each chemical equation involving one or more solid or liquid reactants or products. (a) \(\mathrm{PCl}_{5}(g) \rightleftharpoons \mathrm{PCl}_{3}(l)+\mathrm{Cl}_{2}(g)\) (b) \(2 \mathrm{KClO}_{3}(s) \rightleftharpoons 2 \mathrm{KCl}(s)+3 \mathrm{O}_{2}(g)\) (c) \(\mathrm{HF}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{F}^{-}(a q)\) (d) \(\mathrm{NH}_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{NH}_{4}{ }^{+}(a q)+\mathrm{OH}^{-}(a q)\) Equation Transcription: Text Transcription: \mathrm{PCl}_{5}(g) \rightleftharpoons \mathrm{PCl}_{3}(l)+\mathrm{Cl}_{2}(g) 2 \mathrm{KClO}_{3}(s) \rightleftharpoons 2 \mathrm{KCl}(s)+3 \mathrm{O}_{2}(g)(c) \mathrm{HF}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{F}^{-}(a q) \mathrm{NH}_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{NH}_{4}{ }^{+}(a q)+\mathrm{OH}^{-}(a q)

Write an equilibrium expression for each chemical equation involving one or more solid or liquid reactants or products. (a) \(\mathrm{HCHO}_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{CHO}_{2}{ }^{-}(a q)\) (b) \(\mathrm{CO}_{3}{ }^{2-}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{HCO}_{3}^{-}(a q)+\mathrm{OH}^{-}(a q)\( (c) \(2 \mathrm{C}(\mathrm{s})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{CO}(\mathrm{g})\) (d) \(\mathrm{C}(s)+\mathrm{CO}_{2}(g) \rightleftharpoons 2 \mathrm{CO}(g)\) Equation Transcription: Text Transcription: \mathrm{HCHO}_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{CHO}_{2}{ }^{-}(a q) \mathrm{CO}_{3}{ }^{2-}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{HCO}_{3}^{-}(a q)+\mathrm{OH}^{-}(a q) 2 \mathrm{C}(\mathrm{s})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{CO}(\mathrm{g}) \mathrm{C}(s)+\mathrm{CO}_{2}(g) \rightleftharpoons 2 \mathrm{CO}(g)

Consider the reaction. \(2 \mathrm{H}_{2} \mathrm{~S}(g) \rightleftharpoons 2 \mathrm{H}_{2}(g)+\mathrm{S}_{2}(g)\) Find the mistakes in the equilibrium expression and fix them. \(K_{\mathrm{eq}}=\frac{\left[\mathrm{H}_{2}\right]\left[\mathrm{S}_{2}\right]}{\left[\mathrm{H}_{2} \mathrm{~S}\right]}\) Equation Transcription: Text Transcription: 2 \mathrm{H}_{2} \mathrm{~S}(g) \rightleftharpoons 2 \mathrm{H}_{2}(g)+\mathrm{S}_{2}(g) K_{\mathrm{eq}}=\frac{\left[\mathrm{H}_{2}\right]\left[\mathrm{S}_{2}\right]}{\left[\mathrm{H}_{2} \mathrm{~S}\right]}

Consider the reaction. \(\mathrm{CO}(g)+\mathrm{Cl}_2(g) \rightleftharpoons \mathrm{COCl}_2(g)\) Find the mistake in the equilibrium expression and fix it. \(K_{\text {eq }}=\frac{[\mathrm{CO}]\left[\mathrm{Cl}_2\right]}{\left[\mathrm{COCl}_2\right]}\)

For each equilibrium constant, indicate if you would expect an equilibrium reaction mixture to be dominated by reactants or by products, or to contain significant amounts of both. (a) \(K_{\mathrm{eq}}=5.2 \times 10^{17}\) (b) \(K_{\text {eq }}=1.24\) (c) \(K_{\text {eq }}=3.22 \times 10^{-21}\) (d) \(K_{e q}=0.47\)

For each equilibrium constant, indicate if you would expect an equilibrium reaction mixture to be dominated by reactants or by products, or to contain significant amounts of both. (a) \(K_\mathrm{eq}=0.75\) (b) \(K_\mathrm{eq}=8.5 \times 10^{-7}\) (c) \(K_\mathrm{eq}=1.4 \times 10^{19}\) (d) \(K_\mathrm{eq}=4.7 \times 10^{-9}\) Equation Transcription: Text Transcription: K_eq=0.75 K_eq=8.5 x 10^{-7} K_eq=1.4 x 10^{19} K_eq=4.7 x 10^{-9}

Consider the reaction. \(\mathrm{COCl}_{2}(g) \rightleftharpoons \mathrm{CO}(g)+\mathrm{Cl}_{2}(g)\) An equilibrium mixture of this reaction at a certain temperature has \(\left[\mathrm{COCl}_{2}\right]=0.225 \mathrm{M},[\mathrm{CO}]=0.105 \mathrm{M}\), and \(\left[\mathrm{Cl}_{2}\right]=0.0844 \mathrm{M}\). What is the value of the equilibrium constant at this temperature? Equation Transcription: Text Transcription: \mathrm{COCl}_{2}(g) \rightleftharpoons \mathrm{CO}(g)+\mathrm{Cl}_{2}(g) \left[\mathrm{COCl}_{2}\right]=0.225 \mathrm{M},[\mathrm{CO}]=0.105 \mathrm{M} \left[\mathrm{Cl}_{2}\right]=0.0844 \mathrm{M}

Consider the reaction. \(\mathrm{CO}(g)+2 \mathrm{H}_{2}(g) \rightleftharpoons \mathrm{CH}_{3} \mathrm{OH}(g)\) An equilibrium mixture of this reaction at a certain temperature has \([\mathrm{CO}]=0.105 \mathrm{M},\left[\mathrm{H}_{2}\right]=0.114\mathrm{M}\), and \(\left[\mathrm{CH}_{3} \mathrm{OH}\right]=0.185 \mathrm{M}\). What is the value of the equilibrium constant at this temperature? Equation Transcription: Text Transcription: \mathrm{CO}(g)+2 \mathrm{H}_{2}(g) \rightleftharpoons \mathrm{CH}_{3} \mathrm{OH}(g) [\mathrm{CO}]=0.105 \mathrm{M},\left[\mathrm{H}_{2}\right]=0.114\mathrm{M} \left[\mathrm{CH}_{3} \mathrm{OH}\right]=0.185 \mathrm{M}

Consider the reaction. \(2 \mathrm{H}_{2} \mathrm{~S}(g) \rightleftharpoons 2 \mathrm{H}_{2}(g)+\mathrm{S}_{2}(g)\) An equilibrium mixture of this reaction at a certain temperature has \(\left[\mathrm{H}_{2} \mathrm{~S}\right]=0.562 \mathrm{M},\left[\mathrm{H}_{2}\right]=2.74 \times 10^{-2} \mathrm{M}\), and \(\left[\mathrm{S}_{2}\right]=7.54 \times 10^{-3} \mathrm{M}\). What is the value of the equilibrium constant at this temperature? Equation Transcription: Text Transcription: 2 \mathrm{H}_{2} \mathrm{~S}(g) \rightleftharpoons 2 \mathrm{H}_{2}(g)+\mathrm{S}_{2}(g) \left[\mathrm{H}_{2} \mathrm{~S}\right]=0.562 \mathrm{M},\left[\mathrm{H}_{2}\right]=2.74 \times 10^{-2} \mathrm{M} \left[\mathrm{S}_{2}\right]=7.54 \times 10^{-3} \mathrm{M}

Consider the reaction. \(\mathrm{CO}(g)+\mathrm{H}_{2} \mathrm{O}(g) \rightleftharpoons \mathrm{CO}_{2}(g)+\mathrm{H}_{2}(g)\) An equilibrium mixture of this reaction at a certain temperature has \([\mathrm{CO}]=0.0233 \mathrm{M},\left[\mathrm{H}_{2} \mathrm{O}\right]=0.0115 \mathrm{M},\left[\mathrm{CO}_{2}\right]=0.175 \mathrm{M}\) , and \(\left[\mathrm{H}_{2}\right]=0.0274 \mathrm{M}\). What is the value of the equilibrium constant at this temperature?

Consider the reaction. \(\mathrm{NH}_4 \mathrm{HS}(\mathrm{s}) \rightleftharpoons \mathrm{NH}_3(\mathrm{~g})+\mathrm{H}_2 \mathrm{~S}(g)\) An equilibrium mixture of this reaction at a certain temperature has \(\left[\mathrm{NH}_3\right]=0.278 \mathrm{M}\) and \(\left[\mathrm{H}_2 \mathrm{~S}\right]=0.355 \mathrm{M}\). What is the value of the equilibrium constant at this temperature?

Consider the reaction. \(\mathrm{CaCO}_3(s) \rightleftharpoons \mathrm{CaO}(s)+\mathrm{CO}_2(g)\) An equilibrium mixture of this reaction at a certain temperature has \(\left[\mathrm{CO}_2\right]=0.548\ \mathrm{M}\). What is the value of the equilibrium constant at this temperature?

An equilibrium mixture of the following reaction is found to have \(\left[\mathrm{SbCl}_{3}\right]=0.0255 \mathrm{M}\) and \(\left[\mathrm{Cl}_{2}\right]=0.135 \mathrm{M}\) at \(248^{\circ} \mathrm{C}\). What is the concentration of \(\mathrm{SbCl}_{5}\) ? \(\mathrm{SbCl}_{5}(g) \rightleftharpoons \mathrm{SbCl}_{3}(g)+\mathrm{Cl}_{2}(g) \\ K_{\mathrm{eq}}=4.9 \times 10^{-4} \text { at } 248^{\circ} \mathrm{C}\) Equation Transcription: Text Transcription: [SbCl_3]=0.0255M [Cl_2] =0.135M 248 degree celsius SbCl_5 SbCl_5(g) rightleftharpoons SbCl_3(g)+Cl_2(g) K_eq=4.9 times10^-4 at 248 degree celsius

An equilibrium mixture of the following reaction has \(\left[\mathrm{I}_{2}\right]=0.0205 \mathrm{M}\) at \(1200^{\circ} \mathrm{C}\). What is the concentration of I? \(\mathrm{I}_{2}(g) \rightleftharpoons 2 \mathrm{I}(g)\) \(K_{\mathrm{eq}}=1.1 \times 10^{-2} \text { at } 1200^{\circ} \mathrm{C}\) Equation Transcription: Text Transcription: \left[\mathrm{I}_{2}\right]=0.0205 \mathrm{M} 1200^{\circ} \mathrm{C} \mathrm{I}_{2}(g) \rightleftharpoons 2 \mathrm{I}(g) K_{\mathrm{eq}}=1.1 \times 10^{-2} \text { at } 1200^{\circ} \mathrm{C}

An equilibrium mixture of the following reaction has \(\left[\mathrm{I}_2\right]=0.0112 \mathrm{M}\) and \(\left[\mathrm{Cl}_2\right]=0.0155 \mathrm{M}\) at \(25^{\circ} \mathrm{C}\). What is the concentration of ICl? \(\mathrm{I}_2(g)+\mathrm{Cl}_2(g) \rightleftharpoons 2 \mathrm{ICl}(g)\) \(K_{\mathrm{eq}}=81.9 \text { at } 25^{\circ} \mathrm{C}\)

Consider the reaction: \(\mathrm{H}_{2}(g)+\mathrm{I}_{2}(g) \rightleftharpoons 2 \mathrm{HI}(g)\) Complete the table. Assume that all concentrations are equilibrium concentrations in moles per liter, M. Equation Transcription: Text Transcription: \mathrm{H}_{2}(g)+\mathrm{I}_{2}(g) \rightleftharpoons 2 \mathrm{HI}(g)

Consider this reaction at equilibrium. \(\mathrm{CO}(g)+\mathrm{Cl}_2(g) \rightleftharpoons \mathrm{COCl}_2(g)\) Predict the effect (shift right, shift left, or no effect) of these changes. (a) adding \(\mathrm{Cl}_2\) to the reaction mixture (b) adding \(\mathrm{COCl}_2\) to the reaction mixture (c) adding \(\mathrm{CO}\) to the reaction mixture

Consider this reaction at equilibrium. \(2 \mathrm{BrNO}(g) \rightleftharpoons 2 \mathrm{NO}(g)+\mathrm{Br}_{2}(g)\) Predict the effect (shift right, shift left, or no effect) of these changes. (a) adding BrNO to the reaction mixture (b) adding NO to the reaction mixture (c) adding \(\mathrm{Br}_{2}\) to the reaction mixture Equation Transcription: BrNO NO Text Transcription: 2BrNO(g) rightleftharpoons 2NO(g)+Br_2(g) BrNO NO Br_2

Consider this reaction at equilibrium. \(\mathrm{C}(s)+\mathrm{H}_{2} \mathrm{O}(g) \rightleftharpoons \mathrm{CO}(g)+\mathrm{H}_{2}(g)\) Predict the effect (shift right, shift left, or no effect) of these changes. (a) adding \(\mathrm{C}\) to the reaction mixture (b) condensing \(\mathrm{H}_{2} \mathrm{O}\) and removing it from the reaction mixture (c) adding \(\mathrm{CO}\) to the reaction mixture (d) removing \(\mathrm{H}_{2}\) from the reaction mixture Equation Transcription: Text Transcription: C(s)+H_2O(g) rightleftharpoons CO(g)+H_2(g) C H_2O CO H_2

Consider the effect of a volume change on this reaction at equilibrium. \(\mathrm{I}_2(g)+\mathrm{Cl}_2(g) \rightleftharpoons 2 \mathrm{ICl}(g)\) Predict the effect (shift right, shift left, or no effect) of these changes. (a) increasing the reaction volume (b) decreasing the reaction volume

Consider the effect of a volume change on this reaction at equilibrium. \(\mathrm{I}_{2}(g) \rightleftharpoons 2 \mathrm{I}(g)\) Predict the effect (shift right, shift left, or no effect) of these changes. (a) increasing the reaction volume (b) decreasing the reaction volume Equation Transcription: Text Transcription: I2(g) rightleftharpoons 2I(g)

Consider the effect of a volume change on this reaction at equilibrium. \(2 \mathrm{H}_{2} \mathrm{~S}(g) \rightleftharpoons 2 \mathrm{H}_{2}(g)+\mathrm{S}_{2}(g)\) Predict the effect (shift right, shift left, or no effect) of these changes. (a) increasing the reaction volume (b) decreasing the reaction volume Equation Transcription: Text Transcription: 2H_2 S(g) rightleftharpoons 2H_2(g)+S2(g)

Consider this reaction at equilibrium. \(2 \mathrm{KClO}_3(s) \rightleftharpoons 2 \mathrm{KCl}(s)+3 \mathrm{O}_2(g)\) Predict the effect (shift right, shift left, or no effect) of these changes. (a) adding \(\mathrm{KCl}\) to the reaction mixture (b) adding \(\mathrm{KClO}_3\) to the reaction mixture (c) adding \(\mathrm{O}_2\) to the reaction mixture (d) removing \(\mathrm{O}_2\) from the reaction mixture

Consider the effect of a volume change on this reaction at equilibrium. \(\mathrm{CO}(g)+\mathrm{H}_{2} \mathrm{O}(g) \rightleftharpoons \mathrm{CO}_{2}(g)+\mathrm{H}_{2}(g)\) Predict the effect (shift right, shift left, or no effect) of these changes. (a) increasing the reaction volume (b) decreasing the reaction volume Equation Transcription: Text Transcription: CO(g)+H_2O(g) rightleftharpoons CO_2(g)+H_2(g)

This reaction is endothermic. \(\mathrm{C}(s)+\mathrm{CO}_2(g) \rightleftharpoons 2 \mathrm{CO}(g)\) Predict the effect (shift right, shift left, or no effect) of these changes. (a) increasing the reaction temperature (b) decreasing the reaction temperature

The following reaction is exothermic. \(\mathrm{C}_2 \mathrm{H}_4(g)+\mathrm{Br}_2(g) \rightleftharpoons \mathrm{C}_2 \mathrm{H}_4 \mathrm{Br}_2(g)\) Predict the effect (shift right, shift left, or no effect) of these changes. (a) increasing the reaction temperature (b) decreasing the reaction temperature

This reaction is endothermic. \(\mathrm{I}_{2}(g) \rightleftharpoons 2 \mathrm{I}(g)\) Predict the effect (shift right, shift left, or no effect) of these changes. (a) increasing the reaction temperature (b) decreasing the reaction temperature Equation Transcription: Text Transcription: I_2(g) rightleftharpoons 2I(g)

This reaction is exothermic. \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}(s)+6 \mathrm{O}_{2}(g) \rightleftharpoons 6 \mathrm{CO}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(g)\) Predict the effect (shift right, shift left, or no effect) of these changes. (a) increasing the reaction temperature (b) decreasing the reaction temperature Equation Transcription: Text Transcription: C_6H_12O_6(s)+6O_2(g) rightleftharpoons 6CO_2(g)+6H_2O(g)

Coal, which is primarily carbon, can be converted to natural gas, primarily \( \mathrm{CH}_{4}\), by this exothermic reaction. \(\mathrm{C}(s)+2 \mathrm{H}_{2}(g) \rightleftharpoons \mathrm{CH}_{4}(g)\) If this reaction mixture is at equilibrium, predict the effect (shift right, shift left, or no effect) of these changes. (a) adding more \(C\) to the reaction mixture (b) adding more \(\mathrm{H}_{2}\) to the reaction mixture (c) raising the temperature of the reaction mixture (d) lowering the volume of the reaction mixture (e) adding a catalyst to the reaction mixture Equation Transcription: Text Transcription: CH_4 C(s)+2H_2(g) rightleftharpoons CH_4(g) C H_2

Coal can be used to generate hydrogen gas (a potential fuel) by this endothermic reaction. \(\mathrm{C}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(g) \rightleftharpoons \mathrm{CO}(g)+\mathrm{H}_{2}(g)\) If this reaction mixture is at equilibrium, predict the effect (shift right, shift left, or no effect) of these changes. (a) adding more \(\mathrm{C}\) to the reaction mixture (b) adding more \(\mathrm{H}_{2} \mathrm{O}(g)\) to the reaction mixture (c) raising the temperature of the reaction mixture (d) increasing the volume of the reaction mixture (e) adding a catalyst to the reaction mixture Equation Transcription: Text Transcription: C(s)+H_2O(g) rightleftharpoons CO(g)+H_2(g) H_2O(g)

For each compound, write an equation showing how the compound dissolves in water and write an expression for \(K_\mathrm{sp}\). (a) \(\mathrm{CaSO_4}\) (b) AgCl (c) CuS (d) \(\mathrm{FeCO_3}\) Equation Transcription: Text Transcription: K_sp CaSO_4 FeCO_3

Determine what is wrong with the \(\mathrm{K}_{s p}\) expression for \(\mathrm{Ba}(\mathrm{OH})_{2}\) and correct it. \(K_{s p}=\frac{\left[\mathrm{Ba}(\mathrm{OH})_{2}\right]}{\left[\mathrm{Ba}^{2+}\right]\left[\mathrm{OH}^{-}\right]^{2}}\) Equation Transcription: Text Transcription: K_sp Ba(OH)_2 K_{s p}=\frac{\left[\mathrm{Ba}(\mathrm{OH})_{2}\right]}{\left[\mathrm{Ba}^{2+}\right]\left[\mathrm{OH}^{-}\right]^{2}}

Determine what is wrong with the \(K_\mathrm{sp}\) expression for \(\mathrm{Fe(OH)_2}\) and correct it. \(K_\mathrm{sp}=\mathrm{[Fe^{2+}][OH^-]}\) Equation Transcription: Text Transcription: K_sp Fe(OH)_2 K_sp=[Fe^2+][OH^-]

For each compound, write an equation showing how the compound dissolves in water and write an expression for \(K_\mathrm{sp}\). (a) \(\mathrm{Mg(OH)_2}\) (b) \(\mathrm{FeCO_3}\) (c) PbS (d) \(\mathrm{PbSO_4}\) Equation Transcription: Text Transcription: K_sp Mg(OH)_2 FeCO_3 PbSO_4

A saturated solution of \(\mathrm{MgF_2}\) has \(\mathrm{[Mg^{2+}]=2.6 \times 10^{-4}~ M}\) and \(\mathrm{[F^-]=5.2 \times 10^{-4}~ M}\). What is the value of \(K_\mathrm{sp}\) for \(\mathrm{MgF_2}\)? Equation Transcription: Text Transcription: MgF_2 [Mg^{2+}]=2.6 x 10^{-4} M [F^-]=5.2 x 10^{-4} M K_{sp}

A saturated solution of AgI has \(\mathrm{[Ag^+]=9.2 \times 10^{-9} ~M}\) and \(\mathrm{[I^-]=9.2 \times 10^{-9} ~M}\). What is the value of \(K_\mathrm{sp}\) for AgI? Equation Transcription: Text Transcription: [Ag^+]=9.2 x 10^{-9} M [I^-]=9.2 x 10^{-9} M K_{sp}

A saturated solution of \(\mathrm{PbSO_4}\) has \(\mathrm{[Pb^{2+}]=1.35 \times 10^{-4}~ M}\). What is the concentration of \(\mathrm{SO_4^{~~2-}}\)? Equation Transcription: Text Transcription: PbSO_4 [Pb^{2+}]=1.35 x 10^{-4} M SO_4^{2-}

A saturated solution of \(\mathrm {PbCl_2}\) has \(\mathrm {[Cl^-]=2.86 \times 10^{-2}~ M}\). What is the concentration of \(\mathrm {Pb^{2+}}\)? Equation Transcription: Text Transcription: PbCl_2 [Cl^-]=2.86 x 10^{-2} M Pb^{2+}

Calculate the molar solubility of \(\mathrm {CaCO_3}\). Equation Transcription: Text Transcription: CaCO_3

Calculate the molar solubility of PbS.

Calculate the molar solubility of \(\mathrm {MgCO_3}\). Equation Transcription: Text Transcription: MgCO_3

Calculate the molar solubility of \(\mathrm {CuI}~\left(K_\mathrm{sp}=1.27 \times 10^{-12}\right)\). Equation Transcription: Text Transcription: CuI(K_{sp}=1.27 x 10^{-12})

Complete the table. Assume that all concentrations are equilibrium concentrations in moles per liter, M.

Complete the table. Assume that all concentrations are equilibrium concentrations in moles per liter, M.

Consider the reaction. \(\mathrm{Fe}^{3+}(a q)+\mathrm{SCN}^{-}(a q) \rightleftharpoons \mathrm{FeSCN}^{2+}(a q)\) A solution is made containing initial \([\mathrm{Fe} 3+]=1.0^{*} 10-3 \mathrm{M}\) and initial \([\mathrm{SCN}-]=8.0 * 10-4 \mathrm{M} .\) At equilibrium, \([\mathrm{FeSCN} 2+]=1.7^{*} 10-4 \mathrm{M}\). Calculate the value of the equilibrium constant. Hint: Use the chemical reaction stoichiometry to calculate the equilibrium concentrations of \(\mathrm{Fe} 3+\) and SCN- Equation Transcription: Text Transcription: Fe3+(aq)+SCN-(aq)?FeSCN2+(aq) [Fe3+]=1.0*10-3M [SCN-]=8.0*10-4M [FeSCN2+]=1.7*10-4M Fe3+

Consider the reaction. \(\mathrm{SO}_{2} \mathrm{Cl}_{2}(g) \rightleftharpoons \mathrm{SO}_{2}(g)+\mathrm{Cl}_{2}(g)\) A solution is made containing initial \(\left[\mathrm{SO}_{2} \mathrm{Cl}_{2}\right]=0.020 \mathrm{M}\). At equilibrium, \(\left[\mathrm{Cl}_{2}\right]=1.2 * 10^{-2} \mathrm{M}\). Calculate the value of the equilibrium constant. Hint: Use the chemical reaction stoichiometry to calculate the equilibrium concentrations of \(\mathrm{SO}_{2} \mathrm{Cl} 2_{2}\) and \(\mathrm{SO}_{2}\).

Consider the reaction. \(\mathrm{CO}(g)+\mathrm{Cl}_{2}(g) \rightleftharpoons \mathrm{COCl}_{2}(g) K_{\text {eq }}=6.17 \times 10^{-2} \text { at } 25^{\circ} \mathrm{C}\) A \(3.67-\mathrm{L}\) flask containing an equilibrium reaction mixture has \(\left[\mathrm{H}_{2}\right]=0.104 \mathrm{M}\) and \(\left[\mathrm{I}_{2}\right]=0.0202 \mathrm{M}\). What mass of \(\mathrm{HI}\) in grams is in the equilibrium mixture? Equation Transcription: Text Transcription: mathrm{CO}(g)+\mathrm{Cl}_{2}(g) \rightleftharpoons \mathrm{COCl}_{2}(g) K_{\text {eq }}=6.17 \times 10^{-2} \text { at } 25^{\circ} \mathrm{C} 3.67-L H_2=0.104M I_2=0.0202M HI

Consider the reaction. \(\mathrm{H}_{2}(g)+\mathrm{I}_{2}(g) \rightleftharpoons 2 \mathrm{HI}(g) K_{\text {eq }}=2.9 \times 10^{10} \text { at } 25^{\circ} \mathrm{C}\) A 5.19- \(\mathrm{L}\) flask containing an equilibrium reaction mixture has \([\mathrm{CO}]=1.8 \times 10^{-6} \ \mathrm{M} \text { and }\left[\mathrm{Cl}_2\right]=7.3 \times 10^{-7} \ \mathrm{M}\). What mass of \(\mathrm{COCl}_{2}\) in grams is in the equilibrium mixture?

This reaction is exothermic. \(\mathrm{C}_{2} \mathrm{H}_{4}(g)+\mathrm{Cl}_{2}(g) \rightleftharpoons \mathrm{C}_{2} \mathrm{H}_{4} \mathrm{Cl}_{2}(g)\) If you were a chemist trying to maximize the amount of \(\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{Cl}_{2}\) produced, which of the following might you try? Assume that the reaction mixture reaches equilibrium. (a) increasing the reaction volume (b) removing \(\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{Cl}_{2}\) from the reaction mixture as it forms (c) lowering the reaction temperature (d) adding \(\mathrm{Cl}_{2}\) Equation Transcription: Text Transcription: C_2H_4(g)+Cl_2(g) rightleftharpoons C_2H_4Cl_2(g) C_2H_4Cl_2 Cl_2

This reaction is endothermic. \(\mathrm{C}_{2} \mathrm{H}_{4}(g)+\mathrm{I}_{2}(g) \rightleftharpoons \mathrm{C}_{2} \mathrm{H}_{4} \mathrm{I}_{2}(g)\) If you were a chemist trying to maximize the amount of \(\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{l}_{2}\) produced, which of the following might you try? Assume that the reaction mixture reaches equilibrium. (a) decreasing the reaction volume (b) removing \(\mathrm{I}_{2}\) from the reaction mixture (c) raising the reaction temperature (d) adding \(\mathrm{C}_{2} \mathrm{H}_{4}\) to the reaction mixture Equation Transcription: Text Transcription: C_2H_4(g)+I_2(g) \rightleftharpoons C_2H_4I_2(g) C_2H_4l_2 I_2 C_2H_4

Calculate the molar solubility of CuS. How many grams of CuS are present in 15.0 L of a saturated CuS solution?

Calculate the molar solubility of \(\mathrm {FeCO_3}\). How many grams of \(\mathrm {FeCO_3}\) are present in 15.0 L of a saturated \(\mathrm {FeCO_3}\) solution? Equation Transcription: Text Transcription: FeCO_3

A sample of tap water is found to be 0.025 M in \(\mathrm {Ca^{2+}}\). If 105 mg of \(\mathrm {Na_2SO_4}\) is added to 100.0 mL of the tap water, will any \(\mathrm {CaSO_4}\) precipitate out of solution? Equation Transcription: Text Transcription: Ca^{2+} Na_2SO_4 CaSO_4

If 50.0 mg of \(\mathrm{Na_2CO_3}\) are added to 150.0 mL of a solution that is \(\mathrm{1.5 \times 10^{-3} ~M}\) in \(\mathrm{Mg^{2+}}\), will any \(\mathrm{MgCO_3}\) precipitate from the solution? Equation Transcription: Text Transcription: Na_2CO_3 1.5 x 10^{-3} M Mg^{2+} MgCO_3

The solubility of \(\mathrm{CaCrO}_4\) at \(25^{\circ} \mathrm{C}\) is \(4.15 \mathrm{~g} / \mathrm{L}\). Calculate \(K_{\mathrm{sp}}\) for \(\mathrm{CaCrO}_4\).

The solubility of nickel(II) carbonate at \(\mathrm {25~ ^\circ C}\) is 0.042 g/L. Calculate \(K_\mathrm{sp}\) for nickel(II) carbonate. Equation Transcription: Text Transcription: 25 ^oC K_{sp}

Consider the reaction: \(\mathrm{CaCO}_{3} \rightleftharpoons \mathrm{CaO}(s)+\mathrm{CO}_{2}(g)\) A sample of \(\mathrm{CaCO}_{3}\) is placed into a sealed 0.500-L container and heated to 550 K at which the equilibrium constant is \(4.1^{*} 10^{-4}\). When the reaction has come to equilibrium, what mass of solid CaO is in the container? (Assume that the sample of \(\mathrm{CaCO}_{3}\) was large enough that equilibrium could be achieved.) Equation Transcription: CaCO3 4.1 * 10-4 Text Transcription: CaCO_3 Harpoon CaO(s) + CO_2(g) CaCO_3 4.1 times 10^-4

Consider the reaction: \(\mathrm{NH}_{4} \mathrm{HS}(s) \rightleftharpoons \mathrm{NH}_{3}(g)+\mathrm{H}_{2} \mathrm{~S}(g)\) A sample of pure \(\mathrm{NH}_{4} \mathrm{HS}\) is placed in a sealed 2.0-L container and heated to 550 K at which the equilibrium constant is \(3.5^{*} 10^{-3}\). Once the reaction reaches equilibrium, what mass of \(\mathrm{NH}_{3}\) is in the container? (Assume that the sample of \(\mathrm{NH}_{4} \mathrm{HS}\) was large enough that equilibrium could be achieved.) Equation Transcription: NH4HS 3.5 * 10-3 NH3 Text Transcription: NH_4HS(s) harpoon NH_3(g) + H_2S(g) NH_4HS 3.5 times 10^-3 NH_3

A 2.55-L solution is 0.115 M in \(\mathrm {Mg^{2+}}\). If \(\mathrm {K_2CO_3}\) is added to the solution in order to precipitate the magnesium, what minimum mass of \(\mathrm {K_2CO_3}\) is required to get a precipitate? Equation Transcription: Text Transcription: Mg^{2+} K_2CO_3

A 75.0-L solution is 0.0251 M in \(\mathrm {Ca^{2+}}\). If \(\mathrm {Na_2SO_4}\) is added to the solution in order to precipitate the calcium, what minimum mass of \(\mathrm {Na_2SO_4}\) is required to get a precipitate? Equation Transcription: Text Transcription: Ca^{2+} Na_2SO_4

\(\mathrm{H}_{2}\) and \(\mathrm{I}_{2}\) are combined in a flask and allowed to react according to the reaction: \(\mathrm{H}_{2}(g)+\mathrm{I}_{2}(g) \rightleftharpoons 2 \mathrm{HI}(g)\) Examine the figures (sequential in time) and determine which figure represents the point where equilibrium is reached. Equation Transcription: H2 I2 Text Transcription: H_2 I_2 H_2(g)+I_2(g) harpoon 2 HI(g)

Ethene (\(\mathrm{C}_{2} \mathrm{H}_{4}\)) can be halogenated by the reaction: \(\mathrm{C}_{2} \mathrm{H}_{4}(g)+X_{2}(g) \rightleftharpoons \mathrm{C}_{2} \mathrm{H}_{4} X_{2}(g)\) where \(\mathrm{X}_{2}\) can be \(\mathrm{Cl}_{2}\), \(\mathrm{Br}_{2}\), or \(\mathrm{I}_{2}\). Examine the figures representing equilibrium concentrations of this reaction at the same temperature for the three different halogens. Rank the equilibrium constants for these three reactions from largest to smallest. Equation Transcription: C2H4 X2 Cl2 Br2 I2 Text Transcription: C_2H_4 C_2H_4(g) + X_2(g) harpoon C_2H_4X_2(g) X_2 Cl_2 Br_2 I_2

One of the main components of hard water is \(\mathrm {CaCO_3}\). When hard water evaporates, some of the \(\mathrm {CaCO_3}\) is left behind as a white mineral deposit. Plumbing fixtures in homes with hard water often acquire these deposits over time. Toilets, for example, may develop deposits at the water line as the water in the toilet slowly evaporates away. If water is saturated with \(\mathrm {CaCO_3}\), how much of it has to evaporate to deposit 0.250 g of \(\mathrm {CaCO_3}\)? Hint: Begin by using \(K_\mathrm {sp}\) for \(\mathrm {CaCO_3}\) to determine its solubility. Equation Transcription: Text Transcription: CaCO_3 K_sp

Problem 5Q What factors influence reaction rates? How?