1.) The following reaction was carried out in a 2.50L reaction vessel at 1100 K:
ID: 810851 • Letter: 1
Question
1.) The following reaction was carried out in a 2.50L 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 5.50mol of C, 15.8mol of H2O, 3.10mol of CO, and 8.20mol of H2, what is the reaction quotient Q?
2.) The reaction
2CH4(g)?C2H2(g)+3H2(g)
has an equilibrium constant of K = 0.154.
If 6.70mol of CH4, 4.40mol of C2H2, and 10.90mol of H2 are added to a reaction vessel with a volume of 5.90L , what net reaction will occur?
Options for #2:
a.) The reaction will proceed to the left to establish equilibrium.
b.)The reaction will proceed to the right to establish equilibrium.
c.) No further reaction will occur because the reaction is at equilibrium.
Explanation / Answer
C (s ) + H2O -----------> CO + H2
15.8/2.5 3.10/2.5 8.2/2.5
6.32 1.24 3.28
Qc = [CO][H2]/[H2O]
= 1.24 x3.28/6.32
Reaction quiotient = 0.6435
2) 2CH4 ----------> C2H2 + 3H2
6.7/5.9 4.4/5.9 10.9/5.9
1.14 0.74 1.84
Qc= 0.74x(1.84)3/(1.14)2
3.6
But kc= 0.154
Qc> Kc
So The reaction will proceed to the right to establish equilibrium.
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