- 17.1: Write equilibrium constant expressions for these equilibria. a. N 2...
- 17.2: Challenge Write the chemical equation that has the equilibrium cons...
- 17.3: Write equilibrium constant expressions for these heterogeneous equi...
- 17.4: Challenge Solid iron reacts with chlorine gas to form solid iron(II...
- 17.5: Calculate K eq for the equilibrium in Practice on page 601 using th...
- 17.6: Calculate K eq for the equilibrium in Practice on page 601 using th...
- 17.7: Challenge The reaction COC l 2(g) CO(g) + C l 2 (g) reaches equilib...
- 17.8: Explain how the size of the equilibrium constant relates to the amo...
- 17.9: Compare homogeneous and heterogeneous equilibria
- 17.10: List three characteristics a reaction mixture must have if it is to...
- 17.11: Calculate Determine the value of K eq at 400 K for this equation: P...
- 17.12: Interpret Data The table below shows the value of the equilibrium c...
- 17.13: Explain how a system at equilibrium responds to a stress and list f...
- 17.14: Explain how decreasing the volume of the reaction vessel affects ea...
- 17.15: Decide whether higher or lower temperatures will produce more C H 3...
- 17.16: Demonstrate The table below shows the concentrations of Substances ...
- 17.17: Design a concept map that shows ways in which Le Chteliers principl...
- 17.18: At a certain temperature, K eq = 10.5 for the equilibrium CO(g) + 2...
- 17.19: Challenge In a generic reaction A + B C + D, 1.00 mol of A and 1.00...
- 17.20: Use the data in Table 17.3 to calculate the solubility in mol/L of ...
- 17.21: Challenge The K sp of lead carbonate (PbC O 3) is 7.40 1 0 -14 at 2...
- 17.22: Use K sp values from Table 17.3 to calculate the following. a. [A g...
- 17.23: Calculate the solubility of A g 3P O 4 ( K sp = 2.6 1 0 -18).
- 17.24: Challenge The solubility of silver chloride (AgCl) is 1.86 1 0 -4 g...
- 17.25: Use K sp values from Table 17.3 to predict whether a precipitate wi...
- 17.26: Challenge Will a precipitate form when 250 mL of 0.20M MgC l 2 is a...
- 17.27: List the information you would need in order to calculate the conce...
- 17.28: Explain how to use the solubility product constant to calculate the...
- 17.29: Describe how the presence of a common ion reduces the solubility of...
- 17.30: Explain the difference between K sp and Q sp . Is Q sp an equilibri...
- 17.31: Calculate The K sp of magnesium carbonate (MgC O 3 ) is 2.6 1 0 -9 ...
- 17.32: Design an experiment based on solubilities to demonstrate which of ...
- 17.33: Describe an equilibrium in everyday life that illustrates a state o...
- 17.34: Given the fact that the concentrations of reactants and products ar...
- 17.35: Explain how a person bailing out a row boat with a leak could repre...
- 17.36: Does the following equation represent a homogeneous equilibrium or ...
- 17.37: What is an equilibrium position?
- 17.38: Explain how to write an equilibrium constant expression.
- 17.39: Why should you pay attention to the physical states of reactants an...
- 17.40: Why does a numerically large K eq mean that the products are favore...
- 17.41: What happens to K eq for an equilibrium system if the equation for ...
- 17.42: How can an equilibrium system contain small and unchanging amounts ...
- 17.43: A system, which contains only molecules as reactants and products, ...
- 17.44: Write equilibrium constant expressions for these homogeneous equili...
- 17.45: Write equilibrium constant expressions for these heterogeneous equi...
- 17.46: Heating limestone (CaC O 3 (s)) forms quicklime (CaO(s)) and carbon...
- 17.47: Suppose you have a cube of pure manganese metal measuring 5.25 cm o...
- 17.48: K eq is 3.63 for the reaction A + 2B C. Table 17.5 shows the concen...
- 17.49: When steam is passed over iron filings, solid iron(III) oxide and g...
- 17.50: What is meant by a stress on a reaction at equilibrium?
- 17.51: How does Le Chteliers principle describe an equilibriums response t...
- 17.52: Why does removing a reactant cause an equilibrium shift to the left?
- 17.53: When an equilibrium shifts to the right, what happens to each of th...
- 17.54: Carbonated Beverages Use Le Chteliers principle to explain how a sh...
- 17.55: How would each of the following changes affect the equilibrium posi...
- 17.56: Explain how a temperature increase would affect the equilibrium rep...
- 17.57: A liquid solvent for chlorine is poured into a flask in which the f...
- 17.58: Figure 17.22 shows the following endothermic reaction at equilibriu...
- 17.59: For the equilibrium described in Question 54, what visual change wo...
- 17.60: Given two reactions at equilibrium: a. N 2 (g) + 3 H 2 (g) 2N H 3 (...
- 17.61: Would you expect the numerical value of K eq for the following equi...
- 17.62: Explain how you would regulate the pressure to favor the products i...
- 17.63: Ethylene ( C 2 H 4 ) reacts with hydrogen to form ethane ( C 2 H 6 ...
- 17.64: What does it mean to say that two solutions have a common ion? Give...
- 17.65: Why are compounds such as sodium chloride usually not given K sp va...
- 17.66: X rays Why is barium sulfate a better choice than barium chloride f...
- 17.67: Explain what is happening in Figure 17.23 in terms of Q sp and K sp .
- 17.68: Explain why a common ion lowers the solubility of an ionic compound.
- 17.69: Describe the solution that results when two solutions are mixed and...
- 17.70: Write the K sp expression for lead chromate (PbCr O 4 ), and calcul...
- 17.71: At 350C, K eq = 1.67 1 0 -2 for the reversible reaction 2HI(g) H 2 ...
- 17.72: K sp for scandium fluoride (Sc F 3 ) at 298 K is 4.2 1 0 -18 . Writ...
- 17.73: Will a precipitate form when 62.6 mL of 0.0322M CaC l 2 and 31.3 mL...
- 17.74: Manufacturing Ethyl acetate (C H 3 COOC H 2 C H 3 ), a solvent used...
- 17.75: Ethyl acetate (C H 3 COOC H 2 C H 3 ) is produced in the equilibriu...
- 17.76: How would these equilibria be affected by decreasing the temperatur...
- 17.77: How would simultaneously increasing the temperature and volume of t...
- 17.78: The solubility product constant for lead(II) arsenate (P b 3 (As O ...
- 17.79: Evaluate this statement: A low value for K eq means that both the f...
- 17.80: Food Flavoring Benzaldehyde, known as artificial almond oil, is use...
- 17.81: In the equilibrium system N 2 O 4 (g) 2N O 2 (g), N 2 O 4 is colorl...
- 17.82: Describe the process by which adding potassium hydroxide to a satur...
- 17.83: At 298 K, K sp for cadmium iodate (Cd(I O 3 ) 2 ) equals 2.3 1 0 8 ...
- 17.84: Analyze Suppose that an equilibrium system at a given temperature h...
- 17.85: Evaluate Imagine that you are a chemical engineer designing a produ...
- 17.86: Interpret Data What compound would precipitate first if a 0.500M so...
- 17.87: Apply Smelling salts, sometimes used to revive a person who is unco...
- 17.88: Recognize Cause and Effect Suppose you have 12.56 g of a mixture ma...
- 17.89: Compare and Contrast Which of the two solids, calcium phosphate or ...
- 17.90: Synthesis of Phosgene Phosgene (COC l 2 ) is a toxic gas that is us...
- 17.91: Explain the general trend in ionization energy as you go from left ...
- 17.92: How are the lengths of covalent bonds related to their strength? (C...
- 17.93: How are the chemical bonds in H 2 , O 2 , and N 2 different? (Chapt...
- 17.94: How can you tell if a chemical equation is balanced? (Chapter 9)
- 17.95: What mass of carbon must burn to produce 4.56 L C O 2 gas at STP? (...
- 17.96: Describe a hydrogen bond. What conditions must exist for a hydrogen...
- 17.97: What gas law is exemplified in Figure 17.25? State the law. (Chapte...
- 17.98: When you reverse a thermochemical equation, why must you change the...
- 17.99: What is the sign of the free energy change, G system , for a sponta...
- 17.100: A New Compound Imagine that you are a scientist who has created a u...
- 17.101: Kidney Stones Research the role that solubility plays in the format...
- 17.102: Hard Water The presence of magnesium and calcium ions in water make...
- 17.103: Write the equilibrium constant expression for this equilibrium.
- 17.104: Examine the relationship between K eq and temperature. Use Le Chtel...
- 17.105: Explain how automobile radiators plated with the alloy might help r...
Solutions for Chapter 17: Chemical Equilibrium
Full solutions for Chemistry: Matter & Change | 1st Edition
ISBN: 9780078746376
Since 105 problems in chapter 17: Chemical Equilibrium have been answered, more than 256172 students have viewed full step-by-step solutions from this chapter. Chapter 17: Chemical Equilibrium includes 105 full step-by-step solutions. This expansive textbook survival guide covers the following chapters and their solutions. This textbook survival guide was created for the textbook: Chemistry: Matter & Change, edition: 1. Chemistry: Matter & Change was written by and is associated to the ISBN: 9780078746376.
-
1,2-elimination
An elimination reaction in which a proton from the beta (b) position is removed together with the leaving group, forming a double bond.
-
alkanes.
Hydrocarbons having the general formula CnH2n12, where n 5 1,2, . . . . (24.2)
-
Alkyl group
A group derived by removing a hydrogen from an alkane; given the symbol R!
-
Allene
The compound CH2"C"CH2. Any compound that contains adjacent carbon-carbon double bonds; that is, any molecule that contains a C"C"C functional group.
-
alpha decay
A type of radioactive decay in which an atomic nucleus emits an alpha particle and thereby transforms (or “decays”) into an atom with a mass number 4 less and atomic number 2 less. (Section 21.1)
-
atactic
A polymer in which the repeating units contain chirality centers which are not arranged in a pattern (they have random configurations).
-
Charles’ and Gay-Lussac’s law.
See Charles’ law.
-
condensation polymerization
Polymerization in which molecules are joined together through condensation reactions. (Section 12.8)
-
electromotive force (emf)
A measure of the driving force, or electrical pressure, for the completion of an electrochemical reaction. Electromotive force is measured in volts: 1 V = 1 J>C. Also called the cell potential. (Section 20.4)
-
Glass transition temperature (TG)
The temperature at which a polymer undergoes the transition from a hard glass to a rubbery state
-
group
Elements that are in the same column of the periodic table; elements within the same group or family exhibit similarities in their chemical behavior. (Section 2.5)
-
heterogeneous catalyst
A catalyst that is in a different phase from that of the reactant substances. (Section 14.7)
-
integration
In 1H NMR spectroscopy, the area under a signal indicates the number of protons giving rise to the signal.
-
isothermal process
One that occurs at constant temperature. (Section 19.1)
-
Micelle
A spherical arrangement of organic molecules in water solution clustered so that their hydrophobic parts are buried inside the sphere and their hydrophilic parts are on the surface of the sphere and in contact with water
-
Polynuclear aromatic hydrocarbon (PAH)
A hydrocarbon containing two or more fused benzene rings
-
pure substance
Matter that has a fixed composition and distinct properties. (Section 1.2)
-
Stereochemistry
The study of three-dimensional arrangements of atoms in molecules
-
Steric hindrance
The ability of groups, because of their size, to hinder access to a reaction site within a molecule.
-
Valence-shell electron-pair repulsion (VSEPR)
A method for predicting bond angles based on the idea that electron pairs repel each other and keep as far apart as possible.