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Chapter 13: Q87E (page 760)
Question: What is the minimum mass of CaCO3 required to establish equilibrium at a certain temperature in a 6.50-L container if the equilibrium constant (Kc) is 0.050 for the decomposition reaction of CaCO3 at that temperature?
The minimum mass of CaCO3required is 3.25 g.
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How will an increase in temperature affect each of the following equilibrium? How will a decrease in the volume of the reaction vessel affect each?
\(\begin{gathered} (a)2{H_2}O(g) \rightleftharpoons 2{H_2}(g) + {O_2}(g) \hfill \\ \Delta H = 484kJ \hfill \\ (b){N_2}(g) + 3{H_2}(g) \rightleftharpoons 2N{H_3}(g) \hfill \\ \Delta H = - 92.2kJ \hfill \\ (c)2Br(g) \rightleftharpoons B{r_2}(g) \hfill \\ \Delta H = - 224kJ \hfill \\ (d){H_2}(g) + {I_2}(s) \rightleftharpoons 2HI(g) \hfill \\ \Delta H = 53kJ \hfill \\ \end{gathered}\)
For which of the reactions in Exercise 13.15 does\({K_c}\)(calculated using concentrations) equal\({K_p}\)(calculated using pressures)?
(a) \(C{H_4}(g) + C{l_2} \rightleftharpoons C{H_3}CI(g) + HCI(g)\)
(b) \({N_2}(g) + {O_2}(g)\rightleftharpoons 2NO(g)\)
(c) \(2S{O_2}(\;g) + {O_2}(\;g)\rightleftharpoons 2S{O_3}(\;g)\)
(d) \(BaS{O_3}(s)\rightleftharpoons BaO(s) + S{O_2}(g)\)
(e) \({P_4}(g) + 5{O_2}(g)\rightleftharpoons{P_4}{O_{10}}(s)\)
(f) \(B{r_2}(\;g)\rightleftharpoons 2Br(g)\)
(g) \(C{H_4}(g) + 2{O_2}(g)\rightleftharpoons C{O_2}(g) + 2{H_2}O(l)\)
(h)\(CuS{O_4} \times 5{H_2}O(s)\rightleftharpoons CuS{O_4}(s) + 5{H_2}O(g)\)
A sample of ammonium chloride was heated in a closed container. NH4 Cl (s)⇌ NH3 (g) + HCl(g)at equilibrium, the pressure of NH3 (g)was found to be 1.75 atm. What is the value of the equilibrium constant, Kp, for the decomposition at this temperature?
Question: At 25 °C and at 1 atm, the partial pressures in an equilibrium mixture of N2O4 and NO2 are PN2O4= 0.70 atm and PNO2 = 0.30 atm.
(a) Predict how the pressures of NO2 and N2O4 will change if the total pressure increases to 9.0 atm. Will they increase, decrease, or remain the same?
(b) Calculate the partial pressures of NO2 and N2O4 when they are at equilibrium at 9.0 atm and 25 °C
Question: Consider the equilibrium
4NO2(g) + 6H2 O(g) ⇌ 4NH3(g) + 7O2(g)
(a) What is the expression for the equilibrium constant (Kc) of the reaction?
(b) How must the concentration of NH3 change to reach equilibrium if the reaction quotient is less than the equilibrium constant?
(c) If the reaction were at equilibrium, how would a decrease in pressure (from an increase in the volume of the reaction vessel) affect the pressure of NO2?
(d) If the change in the pressure of NO2 is 28 torr as a mixture of the four gases reaches equilibrium, how much will the pressure of O2 change?
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