?The equilibrium pressure of \(\mathrm{H}_{2}\) over solid uranium and uranium hydride

Explain how the mixing of reactants and products affects the position of chemical equilibrium.

What is the physical justification for not including a pure liquid or solid in the expression for an equilibrium constant?

Consider the reaction A \(\rightarrow\) 2B. Initially 1.50mol A is present and no B. What are the amounts of A and B when the extent of reaction is 0.60mol? Text Transcription: ?

Consider the reaction 2A \(\rightarrow\)B. Initially 1.75mol A and 0.12mol B are present. What are the amounts of A and B when the extent of reaction is 0.30mol? Text Transcription: ?

When the reaction A \(\rightarrow\)2B advances by 0.10mol (i.e. \(\Delta \xi\) = +0.10mol) the molar Gibbs energy of the system changes by ?6.4 kJ \(\mathrm{mol}^{-1}\). What is the Gibbs energy of reaction at this stage of the reaction? Text Transcription: ? ?? mol^?1

When the reaction 2A \(\rightarrow\) B advances by 0.051mol (i.e. \(\Delta \xi\) = +0.051mol) the molar Gibbs energy of the system changes by ?2.41 kJ \(\mathrm{mol}^{-}\). What is the Gibbs energy of reaction at this stage of the reaction? Text Transcription: ? ?? mol^?1

Classify the formation of methane from its elements in their reference states as exergonic or endergonic under standard conditions at 298K.

Classify the formation of liquid benzene from its elements in their reference states as exergonic or endergonic under standard conditions at 298K.

Write the reaction quotient for A + 2B \(\rightarrow\) 3C. Text Transcription: ?

Write the reaction quotient for 2A + B \(\rightarrow\) 2C + D. Text Transcription: ?

Write the equilibrium constant for the reaction \(\mathrm{P}_{4}(\mathrm{s})+6 \mathrm{H}_{2}(\mathrm{g})\) \(\rightleftharpoons 4 \mathrm{PH}_{3}\)(g), with the gases treated as perfect. Text Transcription: P_4(s) + 6H_2(g) 4PH_3

Write the equilibrium constant for the reaction \(\mathrm{CH}_{4}(\mathrm{g})+3 \mathrm{Cl}_{2}(\mathrm{g})\) \(\rightleftharpoons \mathrm{CHCl}_{3}(\mathrm{l})+3 \mathrm{HCl}(\mathrm{g})\) with the gases treated as perfect. Text Transcription: CH_4(g) + 3Cl_2(g) CHCl_3(l) + 3HCl(g)

Use data found in the Resource section to decide which of the following reactions have \(K>1 \text { at } 298 \mathrm{K}: \text { (i) } 2 \mathrm{CH}_{3} \mathrm{CHO}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g})\) \(\rightleftharpoons 2 \mathrm{CH}_{3} \mathrm{COOH}(\mathrm{l}), \text { (ii) } 2 \mathrm{AgCl}(\mathrm{s})+\mathrm{Br}_{2}(\mathrm{l}) \rightleftharpoons 2 \mathrm{AgBr}(\mathrm{s})+\mathrm{Cl}_{2}(\mathrm{~g})\). Text Transcription: K > 1 at 298K: (i) 2CH3CHO(g) + O2(g) 2CH_COOH(l), (ii) 2AgCl(s) + Br_2(l) 2AgBr(s) + Cl_2(g)

Use data found in the Resource section to decide which of the following reactions have \(K<1 \text { at } 298 \mathrm{K}:(\mathrm{i}) \mathrm{Hg}(\mathrm{l})+\mathrm{Cl}_{2}(\mathrm{g}) \rightleftharpoons \mathrm{HgCl}_{2}(\mathrm{s})\), (ii) \(\mathrm{Zn}(\mathrm{s})+\mathrm{Cu}^{2+}(\mathrm{aq}) \rightleftharpoons \mathrm{Zn}^{2+}(\mathrm{aq})+\mathrm{Cu}(\mathrm{s})\) Text Transcription: K < 1 at 298K: (i) Hg(l) + Cl2(g) HgCl2(s) Zn(s) + Cu2+(aq) Zn2+ (aq) + Cu(s)

One reaction has a standard Gibbs energy of ?320 kJ\(\mathrm{mol}^{-1}\) and a second reaction has a standard Gibbs energy of ?55 kJ\(\mathrm{mol}^{-1}\)1, both at 300K. What is the ratio of their equilibrium constants at 300K? Text Transcription: mol^?1

One reaction has a standard Gibbs energy of ?200 kJ\(\mathrm{mol}^{-1}\) and a second reaction has a standard Gibbs energy of +30 kJ\(\mathrm{mol}^{-1}\), both at 300K. What is the ratio of their equilibrium constants at 300K? Text Transcription: mol^?1

The standard Gibbs energy of the reaction \(\mathrm{N}_{2}(\mathrm{g})+3 \mathrm{H}_{2}(\mathrm{g}) \rightarrow 2 \mathrm{NH}_{3}(\mathrm{g})\) is ?32.9 kJ\(\mathrm{mol}^{-1}\) at 298K. What is the value of \(\Delta_{\mathrm{r}} G\) when Q = (i) 0.010, (ii) 1.0, (iii) 10.0, (iv) 100 000, (v) 1 000 000? Estimate (by interpolation) the value of K from the values you calculate. What is the actual value of K? Text Transcription: N_2(g) + 3H_2(g) ? 2NH_3(g) mol^?1 ?r G

The standard Gibbs energy of the reaction \(2 \mathrm{NO}_{2}(\mathrm{g}) \rightarrow \mathrm{N}_{2} \mathrm{O}_{4}(\mathrm{g})\) is ?4.73 kJ\(\mathrm{mol}^{-}\) at 298K. What is the value of \(\Delta_{r} G\) when Q = (i) 0.10, (ii) 1.0, (iii) 10, (iv) 100? Estimate (by interpolation) the value of K from the values you calculate. What is the actual value of K? Text Transcription: 2NO_2(g) ? N_2O_4(g) mol^?1 ?rG

At 2257K and 1.00bar total pressure, water is 1.77 per cent dissociated at equilibrium by way of the reaction \(2 \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightleftharpoons 2 \mathrm{H}_{2}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g})\). Calculate K. Text Transcription: 2H_2O(g) 2H_2(g) + O_2(g)

For the equilibrium, \(\mathrm{N}_{2} \mathrm{O}_{4}(\mathrm{g}) \rightleftharpoons 2 \mathrm{NO}_{2}(\mathrm{g})\), the degree of dissociation, ?, at 298K is 0.201 at 1.00bar total pressure. Calculate K. Text Transcription: N_2O_4(g) 2NO_2(g)

Establish the relation between K and \(K_{c}\)Kc for the reaction \(\mathrm{H}_{2} \mathrm{CO}(\mathrm{g})\) \(\rightleftharpoons \mathrm{CO}(\mathrm{g})+\mathrm{H}_{2}(\mathrm{g})\). Text Transcription: K_c H_2CO(g) CO(g) + H_2(g)

Establish the relation between K and \(K_{c}\) for the reaction \(3 \mathrm{N}_{2}(\mathrm{g})+\) \(\mathrm{H}_{2}(\mathrm{g}) \rightleftharpoons 2 \mathrm{HN}_{3}(\mathrm{g})\). ________________ Text Transcription: k_c 3N_2(g) +H_2(g) 2HN_3(g)

In the gas-phase reaction \(2 \mathrm{A}+\mathrm{B} \rightleftharpoons 3 \mathrm{C}+2 \mathrm{D}\), it was found that, when 1.00mol A, 2.00mol B, and 1.00mol D were mixed and allowed to come to equilibrium at \(25^{\circ} \mathrm{C}\), the resulting mixture contained 0.90mol C at a total pressure of 1.00bar. Calculate (i) the mole fractions of each species at equilibrium, (ii) K, and (iii) \(\Delta_{\mathrm{r}} G^{\circ}\) Text Transcription: 2A + B 3C + 2D 25 °C ?rG?

E6A.11(b) In the gas-phase reaction \(\mathrm{A}+\mathrm{B} \rightleftharpoons \mathrm{C}+2 \mathrm{D}\), it was found that, when 2.00mol A, 1.00mol B, and 3.00mol D were mixed and allowed to come to equilibrium at \(25^{\circ} \mathrm{C}\), the resulting mixture contained 0.79mol C at a total pressure of 1.00bar. Calculate (i) the mole fractions of each species at equilibrium, (ii) K, and (iii) \(\Delta_{\mathrm{r}} G^{e}\). Text Transcription: A + B C + 2D 25 °C ?rG?

The standard reaction Gibbs energy of the isomerization of borneol \(\left(\mathrm{C}_{10} \mathrm{H}_{17} \mathrm{OH}\right)\) to isoborneol in the gas phase at 503K is +9.4 kJ\(\mathrm{mol}^{-1}\). Calculate the reaction Gibbs energy in a mixture consisting of 0.15mol of borneol and 0.30mol of isoborneol when the total pressure is 600Torr. Text Transcription: C_10H_17OH mol^?1

The equilibrium pressure of \(\mathrm{H}_{2}\) over solid uranium and uranium hydride, \(\mathrm{UH}_{3}\), at 500K is 139Pa. Calculate the standard Gibbs energy of formation of \(\mathrm{UH}_{3}\)(s) at 500K. Text Transcription: H_2 UH_3

The standard Gibbs energy of formation of \(\mathrm{NH}_{3}(\mathrm{g})\) is ?16.5 kJ\(\mathrm{mol}^{-1}\) at 298K. What is the corresponding reaction Gibbs energy when the partial pressures of the \(\mathrm{N}_{2}, \mathrm{H}_{2}\), and NH3 (treated as perfect gases) are 3.0bar, 1.0bar, and 4.0bar, respectively? What is the spontaneous direction of the reaction in this case? Text Transcription: NH_3(g) mol^?1 N_2 H_2

E6A.13(b) The standard Gibbs energy of formation of \(\mathrm{PH}_{3}(\mathrm{g})\) is +13.4 kJ\(\mathrm{mol}^{-1}\) at 298K. What is the corresponding reaction Gibbs energy when the partial pressures of the \(\mathrm{H}_{2}\) and \(\mathrm{PH}_{3}\) (treated as perfect gases) are 1.0bar and 0.60bar, respectively? What is the spontaneous direction of the reaction in this case? Text Transcription: PH_3(g) mol^?1 H_2 PH_3

For \(\mathrm{CaF}_{2}(\mathrm{s}) \rightleftharpoons \mathrm{Ca}^{2+}(\mathrm{aq})+2 \mathrm{F}^{-}(\mathrm{aq})\), \(K=3.9 \times 10^{-11} \text { at } 25^{\circ} \mathrm{C}\) and the standard Gibbs energy of formation of \(\mathrm{CaF}_{2}(\mathrm{s})\) is ?1167 kJ\(\mathrm{mol}^{-}\). Calculate the standard Gibbs energy of formation of \(\(\mathrm{CaF}_{2}(\mathrm{aq})\\). Text Transcription: CaF2(s) Ca2+(aq) + 2F?(aq) K = 3.9 ×10?11 at 25 °C CaF_2(s) CaF_2(aq) mol^?1

For \(\mathrm{PbI}_{2}(\mathrm{s}) \rightleftharpoons \mathrm{Pb}^{2+}(\mathrm{aq})+2 \mathrm{I}^{-}(\mathrm{aq})\), \(K=1.4 \times 10^{-8} \text { at } 25^{\circ} \mathrm{C}\) and the standard Gibbs energy of formation of \(\mathrm{PbI}_{2}(\mathrm{s})\) is ?173.64 kJ\(\mathrm{mol}^{-1}\). Calculate the standard Gibbs energy of formation of \(\mathrm{PbI}_{2}(\mathrm{aq})\). Text Transcription: PbI_2(s) Pb_2+(aq) + 2 I?(aq) K = 1.4 × 10?8 at 25 °C PbI_2(s) PbI_2(aq) mol^?1

The equilibrium constant for the reaction, \(\mathrm{I}_{2}(\mathrm{s})+\mathrm{Br}_{2}(\mathrm{g}) \rightleftharpoons 2 \operatorname{IBr}(\mathrm{g})\) is 0.164 at \(25^{\circ} \mathrm{C}\). (a) Calculate \(\Delta_{T} G^{\ominus}\) for this reaction. (b) Bromine gas is introduced into a container with excess solid iodine. The pressure and temperature are held at 0.164 atm and \(25^{\circ} \mathrm{C}\), respectively. Find the partial pressure of IBr(g) at equilibrium. Assume that all the bromine is in the gaseous form and that the vapour pressure of iodine is negligible. (c) In fact, solid iodine has a measurable vapour pressure at \(25^{\circ} \mathrm{C}\). In this case, how would the calculation have to be modified? Text Transcription: I_2(s) + Br_2(g) 2 IBr(g) 25 °C ?rG?

P6A.2 Calculate the equilibrium constant of the reaction CO(g) + \(\mathrm{H}_{2}(\mathrm{g}) \rightleftharpoons \mathrm{H}_{2} \mathrm{CO}(\mathrm{g})\) given that, for the production of liquid methanal (formaldehyde), \(\Delta_{\mathrm{r}} G^{6}\)= +28.95 kJ\(\mathrm{mol}^{-1}\) at 298K and that the vapour pressure of methanal is 1500Torr at that temperature. Text Transcription: H_2(g) H_2CO(g) ?rG? mol^?1

A sealed container was filled with 0.300mol \(\mathrm{H}_{2}(\mathrm{g})\), 0.400mol \(\mathrm{I}_{2}(\mathrm{g})\), and 0.200mol HI(g) at 870K and total pressure 1.00bar. Calculate the amounts of the components in the mixture at equilibrium given that K = 870 for the reaction \(\mathrm{H}_{2}(\mathrm{g})+\mathrm{I}_{2}(\mathrm{g}) \rightleftharpoons 2 \mathrm{HI}(\mathrm{g})\). Text Transcription: H_2(g) I_2(g) H_2(g) + I_2(g) 2HI(g)

Nitric acid hydrates have received much attention as possible catalysts for heterogeneous reactions that bring about the Antarctic ozone hole.Standard reaction Gibbs energies at 190K are as follows: (i) \(\mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightarrow \mathrm{H}_{2} \mathrm{O}(\mathrm{s})\) \(\Delta_{\mathrm{r}} G^{\ominus}=-23.6 \mathrm{kJ} \mathrm{mol}^{-1}\) (ii) \(\mathrm{H}_{2} \mathrm{O}(\mathrm{g})+\mathrm{HNO}_{3}(\mathrm{g}) \rightarrow \mathrm{HNO}_{3} \cdot \mathrm{H}_{2} \mathrm{O}(\mathrm{s})\) \(\Delta_{r} G^{\ominus}=-57.2 \mathrm{kJ} \mathrm{mol}^{-1}\) (iii) \(2 \mathrm{H}_{2} \mathrm{O}(\mathrm{g})+\mathrm{HNO}_{3}(\mathrm{g}) \rightarrow \mathrm{HNO}_{3} \cdot 2 \mathrm{H}_{2} \mathrm{O}(\mathrm{s})\) \(\Delta_{\mathrm{r}} G^{\ominus}=-85.6 \mathrm{kJ} \mathrm{mol}^{-1}\) (iv) \(3 \mathrm{H}_{2} \mathrm{O}(\mathrm{g})+\mathrm{HNO}_{3}(\mathrm{g}) \rightarrow \mathrm{HNO}_{3} \cdot 3 \mathrm{H}_{2} \mathrm{O}(\mathrm{s})\) \(\Delta_{\mathrm{r}} G^{\ominus}=-112.8 \mathrm{kJ} \mathrm{mol}^{-1}\) Which solid is thermodynamically most stable at 190 K if \(p_{\mathrm{H}_{2} \mathrm{O}}=0.13 \mu \mathrm{bar}\) and \(P_{\mathrm{HNO}_{3}}\) = 0.41nbar? Hint: Try computing \(\Delta_{r} G\) for each reaction under the prevailing conditions. If more than one solid form spontaneously, then examine \(\Delta_{r} G\) for the conversion of one solid to another. Text Transcription: H_2O(g) ? H_2O(s) ?rG? = ?23.6 kJmol^?1 H_2O(g) + HNO_3(g) ? HNO_3 ?H_2O(s) ?rG? = ?57.2 kJmol^?1 2H_2O(g) + HNO_3(g) ? HNO_3 ? 2H_2O(s) ?rG?= ?85.6 kJmol^?1 3H_2O(g) + HNO_3(g) ? HNO_3 ? 3H2O(s) ?rG? = ?112.8 kJmol^?1 p_H_2O = 0.13?bar pHNO_3 ?rG

Express the equilibrium constant of a gas-phase reaction A + 3B \(\rightleftharpoons 2 \mathrm{C}\) in terms of the equilibrium value of the extent of reaction, \(\xi\), given that initially A and B were present in stoichiometric proportions. Find an expression for \(\xi\), as a function of the total pressure, p, of the reaction mixture and sketch a graph of the expression obtained. Text Transcription: 2C ?

Consider the equilibrium \(\mathrm{N}_{2} \mathrm{O}_{4}(\mathrm{g}) \rightleftharpoons 2 \mathrm{NO}_{2}(\mathrm{g})\). From the tables of data in the Resource section, assess the contributions of \(\Delta_{\mathrm{r}} H^{\ominus} \text { and } \Delta_{\mathrm{r}} S^{\ominus}\) to the value of K at 298K. Text Transcription: N_2O_4(g) 2NO)2(g) ?rH? and ?rS?