1. A 0.100-mol sample of NO2 was placed in a 10.0-L container and heated to 750 K. The total pressure of the equilibrium mixture as a result of the decomposition 2NO2(g) â 2NO(g) + O2(g) was 0.827 bar. What is the value of K at this temperature?
2. A 0.0100-mol sample of NO2 was placed in the container described in Problem 1, and equilibrium was established at 750 K. What is the degree of dissociation? Compare the value to that for the 0.100-mol NO2 sample in Problem 1.
3. Repeat the calculation of Problem 2 for a 0.0100-mol sample of NO2 mixed with 0.100 mol of an inert gas. The total pressure of the equilibrium mixture is 0.712 bar. Assume ideal gas behavior. What is the effect of the inert gas?
4. The equilibrium constant (Kw) for the equation H2O(l) â H+(aq) + OH-(aq) was measured at several temperatures. Determine ârHø(298K) for the reaction using the following data:
T (ËC) 0 25 40 60
Kw 1.15 x 10-15 1.00 x 10-14 2.95 x 10-14 9.55 x 10-14
1. A 0.100-mol sample of NO2 was placed in a 10.0-L container and heated to 750 K. The total pressure of the equilibrium mixture as a result of the decomposition 2NO2(g) â 2NO(g) + O2(g) was 0.827 bar. What is the value of K at this temperature?
2. A 0.0100-mol sample of NO2 was placed in the container described in Problem 1, and equilibrium was established at 750 K. What is the degree of dissociation? Compare the value to that for the 0.100-mol NO2 sample in Problem 1.
3. Repeat the calculation of Problem 2 for a 0.0100-mol sample of NO2 mixed with 0.100 mol of an inert gas. The total pressure of the equilibrium mixture is 0.712 bar. Assume ideal gas behavior. What is the effect of the inert gas?
4. The equilibrium constant (Kw) for the equation H2O(l) â H+(aq) + OH-(aq) was measured at several temperatures. Determine ârHø(298K) for the reaction using the following data:
T (ËC) 0 25 40 60
Kw 1.15 x 10-15 1.00 x 10-14 2.95 x 10-14 9.55 x 10-14
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