Consider the following reaction: 2NO(g) + 2H2(g) = N2(g) + 2H2O(g) Initially, a mixture of 0.200 mol NO(g), 0.150 mol H2(g), 0.100 mol H20(g) was allowed to reach equilibrium in a 2.50-L flask at a certain temperature. At equilibrium, the concentration of NO was found to be 0.034 M. a. Determine the value of the equilibrium constant, K: Answer: Solution: b. Assuming that the temperature is 200°C, what will be the value of K,?

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2. Consider the following reaction:
2NO(g) + 2H2(g) N2(g) + 2H2O(g)
Initially, a mixture of 0.200 mol NO(g). 0.150 mol H2(g), 0.100 mol H20(g) was allowed to reach
equilibrium in a 2.50-L flask at a certain temperature. At equilibrium, the concentration of NO was
found to be 0.034 M.
a. Determine the value of the equilibrium constant, K:
Answer:
Solution:
b. Assuming that the temperature is 200°C, what will be the value of K,?
Answer:
Solution:
Transcribed Image Text:2. Consider the following reaction: 2NO(g) + 2H2(g) N2(g) + 2H2O(g) Initially, a mixture of 0.200 mol NO(g). 0.150 mol H2(g), 0.100 mol H20(g) was allowed to reach equilibrium in a 2.50-L flask at a certain temperature. At equilibrium, the concentration of NO was found to be 0.034 M. a. Determine the value of the equilibrium constant, K: Answer: Solution: b. Assuming that the temperature is 200°C, what will be the value of K,? Answer: Solution:
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