1. The following reaction was carried out in a 4.00L reaction vessel at 1100 K:
ID: 843594 • Letter: 1
Question
1. The following reaction was carried out in a 4.00L reaction vessel at 1100 K:
C(s)+H2O(g)?CO(g)+H2(g)
If during the course of the reaction, the vessel is found to contain 6.50mol of C, 13.4mol of H2O, 4.00mol of CO, and 8.60mol of H2, what is the reaction quotient Q? Answer numerically
2. A mixture initially contains A, B, and C in the following concentrations: [A] = 0.650M , [B] = 1.05M , and [C] = 0.450M . The following reaction occurs and equilibrium is established:
A+2B?C
At equilibrium, [A] = 0.500M and [C] = 0.600M . Calculate the value of the equilibrium constant, Kc. Answer numerically.
Explanation / Answer
1) C(s)+H2O(g)?CO(g)+H2(g)
Q = [C0] [H2] / [H20]
solids should be neglected
[C0] = moles / volume = 4/4 = 1
[H2] = 8.60 / 4 = 2.15
[H20] = 13.4 /4 = 3.35
Q= 1 x 2.15 / 3.35
Q= 0.64
2) A+2B?C
inital [A ] , [B] and [C] are 0.65 , 1.05 and 0.45
at equilbrium [ A] , [B] and [ C] are 0.65 - x , 1.05 -2x and 0.45 + x
Give [C] eq = 0.6
so 0.45 + x = 0.6
x = 0.15
so
[B] eq = 1.05 - 2x 0.15
[B] eq = 0.75
Kc = [ C] / [B]^2 [ A]
Kc = 0.6 / ( 0.75)^2 x 0.5
Kc = 2.13
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