1)Consider the following reaction: 2 HI (g) <=> H? (g) + I? (g) When 4.00 moles
ID: 1046012 • Letter: 1
Question
1)Consider the following reaction:
2 HI (g) <=> H? (g) + I? (g)
When 4.00 moles of HI were put on a container of 5.00 L at 458 degrees, we found that the mix in equilibrium contained 0.442 moles of I?. Determine the value of Kc.
2)The constant of equilibrium for the following reaction is 1.0E-5 at 1500 K.
N? (g) + O? (g) <=> 2NO (g)
If 0.750M of N? y 0.750M of O? are put in the same container and are permitted to reach equilibrium at 1500K, what are the concentrations in equilibrium of all the species?
Explanation / Answer
1.
2 HI (g) <=> H? (g) + I? (g)
Initial [HI] = moles / volume = 4.00 / 5.00 = 0.800 M
At equilibrium, [H2] = [I2] = 0.442 / 5.00 = 0.0884 M
At equilibrium, [HI] = [ 4.00 - ( 2 * 0.442 ) ] / 5.00 = 0.623 M
Therefore,
K = [H2][I2] / [HI]2
K = (0.0884 * 0.0884) / (0.623)2
K = 0.0201
K = 2.01 * 10-2
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