Consider the following equilibrium for decomposition reaction of

water into elemental gases:

2 H2O(g) â 2 H2(g) + O2(g)

Assuming ideal gas behavior and the âÎ¼ Ì for this reaction is known to be 120kJ/mol at 2500 K, what is the partial pressure (in bar) for O2(g) in a 10 L container if the reaction initially started with 1.5 moles of H2O and no products?

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4. For the reaction H2(g) + 1/2O2(g) --> H2O(g) the heat of formation of H2O(g) at 298 K is -241.8

kJ/mol. If 1.4756 moles of H2(g) and 6.6495 moles of O2(g), initially at 298 K, are ignited in an

adiabatic constant pressure (P=1 bar) vessel calculate the final temperature of the gas mixture.

Assume the heat capacities of the gases are constant and are given in Appendix B of your text.

I think this is a limiting reagent problem. Please show steps!

Please answer and explain!

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 ârHÃ¸(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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