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Problem 61e
Consider the following equilibrium, for which Ξπ»<0
2 SO2(π) + O2(π) β 2 SO3(π)
(e) the total pressure of the system is increased by adding a noble gas
Problem 61f
Consider the following equilibrium, for which Ξπ»<0
2 SO2(π) + O2(π) β 2 SO3(π)
(f) How will each of the following changes affect an equilibrium mixture of the three gases: SO3(π) is removed from the system?
Problem 62a,b,c
Consider the reaction 4 NH3(π) + 5 O2(π) β 4 NO(π) + 6 H2O(π), Ξπ» = β904.4 kJ Does each of the following increase, decrease, or leave unchanged the yield of NO at equilibrium? (a) increase [NH3] (b) increase [H2O] (c) decrease [O2]
Problem 62d
Consider the reaction 4 NH3(π) + 5 O2(π) β 4 NO(π) + 6 H2O(π), Ξπ» = β904.4 kJ Does each of the following increase, decrease, or leave unchanged the yield of NO at equilibrium? (d) decrease the volume of the container in which the reaction occurs
Problem 62e
Consider the reaction 4 NH3(π) + 5 O2(π) β 4 NO(π) + 6 H2O(π), Ξπ» = β904.4 kJ Does each of the following increase, decrease, or leave unchanged the yield of NO at equilibrium? (e) add a catalyst
Problem 62f
Consider the reaction 4 NH3(π) + 5 O2(π) β 4 NO(π) + 6 H2O(π), Ξπ» = β904.4 kJ Does each of the following increase, decrease, or leave unchanged the yield of NO at equilibrium? (f) increase temperature.
- How do the following changes affect the value of the equilibrium constant for a gas-phase exothermic reaction: (a) removal of a reactant, (b) removal of a product?
Problem 63
- For a certain gas-phase reaction, the fraction of products in an equilibrium mixture is increased by either increasing the temperature or by increasing the volume of the reaction vessel. Does the balanced chemical equation have more molecules on the reactant side or product side?
Problem 64
Problem 65a
Consider the following equilibrium between oxides of nitrogen 3 NO(g) β NO2(g) + N2O(g) (a) At constant temperature, would a change in the volume of the container affect the fraction of products in the equilibrium mixture?
Problem 66a
Methanol (CH3OH) can be made by the reaction of CO with H2: CO(π) + 2 H2(π) β CH3OH(π) (a) Use thermochemical data in Appendix C to calculate ΞHΒ° for this reaction.
Problem 66b
Methanol (CH3OH) can be made by the reaction of CO with H2: CO(π) + 2 H2(π) β CH3OH(π) (b) To maximize the equilibrium yield of methanol, would you use a high or low temperature?
Problem 66c
Methanol (CH3OH) can be made by the reaction of CO with H2: CO(π) + 2 H2(π) β CH3OH(π) (c) To maximize the equilibrium yield of methanol, would you use a high or low pressure?
Problem 67
Ozone, O3, decomposes to molecular oxygen in the stratosphere according to the reaction 2 O3(π) βΆ 3 O2(π). Would increasing the pressure by decreasing the size of the reaction vessel favor the formation of ozone or of oxygen?
Problem 69a
(a) Is the dissociation of fluorine molecules into atomic fluorine, F2(π) β 2 ββF(π), an exothermic or endothermic process?
Problem 69b
(b) If the temperature is raised by 100 K, does the equilibrium constant for this reaction increase or decrease?
Problem 69c
(c) If the temperature is raised by 100 K, does the forward rate constant kf increase by a larger or smaller amount than the reverse rate constant kr?
- Both the forward reaction and the reverse reaction in the following equilibrium are believed to be elementary steps: CO(g) + Cl2(g) Ξ COCl(g) + Cl(g). At 25 _x001F_C, the rate constants for the forward and reverse reactions are 1.4 * 10^-28 M^-1 s^-1 and 9.3 * 10^10 M^-1 s^-1, respectively. (a) What is the value for the equilibrium constant at 25 _x001F_C? (b) Are reactants or products more plentiful at equilibrium?
Problem 71
- A mixture of CH4 and H2O is passed over a nickel catalyst at 1000 K. The emerging gas is collected in a 5.00-L flask and is found to contain 8.62 g of CO, 2.60 g of H2, 43.0 g of CH4, and 48.4 g of H2O. Assuming that equilibrium has been reached, calculate Kc and Kp for the reaction CH4(g) + H2O(g) β CO(g) + 3H2(g).
Problem 73
Problem 74a
When 2.00 mol of SO2Cl2 is placed in a 2.00-L flask at 303 K, 56% of the SO2Cl2 decomposes to SO2 and Cl2: SO2Cl2(g) β SO2(g) + Cl2(g) (a) Calculate Kc for this reaction at this temperature.
Problem 74c
When 2.00 mol of SO2Cl2 is placed in a 2.00-L flask at 303 K, 56% of the SO2Cl2 decomposes to SO2 and Cl2: SO2Cl2(g) β SO2(g) + Cl2(g) (c) According to Le ChΓ’telier's principle, would the percent of SO2Cl2 that decomposes increase, decrease or stay the same if the mixture were transferred to a 15.00-L vessel?
- The value of the equilibrium constant Kc for the reaction N2(g) + 3 H2(g) β 2 NH3(g) changes in the following manner as a function of temperature: Temperature (Β°C) Kc 300 9.6 400 0.50 500 0.058. (b) Use the standard enthalpies of formation given in Appendix C to determine the ΞH for this reaction at standard conditions. Does this value agree with your prediction from part (a)?
Problem 75
Problem 76b
A sample of nitrosyl bromide (NOBr) decomposes according to the equation 2 NOBr(π) β 2 NO(π) + Br2(π) An equilibrium mixture in a 5.00-L vessel at 100Β°C contains 3.22 g of NOBr, 2.46 g of NO, and 6.55 g of Br2. (b) What is the total pressure exerted by the mixture of gases?
Problem 76c
A sample of nitrosyl bromide (NOBr) decomposes according to the equation 2 NOBr(π) β 2 NO(π) + Br2(π) An equilibrium mixture in a 5.00-L vessel at 100Β°C contains 3.22 g of NOBr, 2.46 g of NO, and 6.55 g of Br2. (c) What was the mass of the original sample of NOBr?
Problem 77c
Consider the hypothetical reaction A(π) β 2 B(π). A flask is charged with 0.75 atm of pure A, after which it is allowed to reach equilibrium at 0Β°C. At equilibrium, the partial pressure of A is 0.36 atm. (c) To maximize the yield of product B, would you make the reaction flask larger or smaller?
Problem 78b
As shown in Table 15.2, the equilibrium constant for the reaction N2(g) + 3 H2(g) β 2 NH3(g) is Kp = 4.34 Γ 10-3 at 300Β°C. Pure NH3 is placed in a 1.00-L flask and allowed to reach equilibrium at this temperature. There are 1.05 g NH3 in the equilibrium mixture. (b) What was the initial mass of ammonia placed in the vessel?
- For the equilibrium 2 IBr(g) β I2(g) + Br2(g), Kp = 8.5 * 10^-3 at 150 _x001F_C. If 0.025 atm of IBr is placed in a 2.0-L container, what is the partial pressure of all substances after equilibrium is reached?
Problem 79
Problem 80b
For the equilibrium PH3BCl3(π ) β PH3(π) + BCl3(π) πΎπ = 0.052 at 60Β°C. (b) A closed 1.500-L vessel at 60Β°C is charged with 0.0500 g of BCl3(π); 3.00 g of solid PH3BCl3 is then added to the flask, and the system is allowed to equilibrate. What is the equilibrium concentration of PH3?
- Solid NH4SH is introduced into an evacuated flask at 24 _x001F_C. The following reaction takes place: NH4SH(s) β NH3(g) + H2S(g). At equilibrium, the total pressure (for NH3 and H2S taken together) is 0.614 atm. What is Kp for this equilibrium at 24 _x001F_C?
Problem 81
Problem 82
A 0.831-g sample of SO3 is placed in a 1.00-L container and heated to 1100 K. The SO3 decomposes to SO2 and O2: 2SO3(π) β 2 SO2(π) + O2(π) At equilibrium, the total pressure in the container is 1.300 atm. Find the values of πΎπ and πΎπ for this reaction at 1100 K.
Problem 84b
Nitric oxide (NO) reacts readily with chlorine gas as follows: 2 NO(π) + Cl2(π) β 2 NOCl(π) At 700 K, the equilibrium constant πΎπ for this reaction is 0.26. For each of the following mixtures at this temperature, indicate whether the mixture is at equilibrium, or, if not, whether it needs to produce more products or reactants to reach equilibrium. (b) πNO = 0.12atm, πCl2 = 0.10atm, πNOCl = 0.050atm