The following reaction was carried out in a 2.50 L reaction vessel at 1100 K: C(
ID: 473926 • Letter: T
Question
The following reaction was carried out in a 2.50 L 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 5.75 mol of C, 14.4 mol of H2O, 3.50 mol of CO, and 8.70 mol of H2, what is the reaction quotient Q? Enter the reaction quotient numerically.
The reaction
2CH4(g)C2H2(g)+3H2(g)
has an equilibrium constant of K = 0.154.
If 6.30 mol of CH4, 4.05 mol of C2H2, and 10.60 mol of H2 are added to a reaction vessel with a volume of 5.60 L , what net reaction will occur?
The reaction
has an equilibrium constant of = 0.154.
If 6.30 of , 4.05 of , and 10.60 of are added to a reaction vessel with a volume of 5.60 , what net reaction will occur?
The reaction will proceed to the left to establish equilibrium. The reaction will proceed to the right to establish equilibrium. No further reaction will occur because the reaction is at equilibrium.Explanation / Answer
For the given reaction,
C(s) + H2O(g) <==> CO(g)
Reaction quotient,
Q = [CO][H2]/[C][H2O]
with,
[CO] = 3.50 mol/2.50 L = 1.40 M
[C] = 5.75 mol/2.50 L = 2.30 M
[H2O] = 14.4 mol/2.50 L = 5.76 M
[H2] = 8.70 mol/2.50 L = 3.48 M
we get,
Q = 1.40 x 3.48/2.30 x 5.76 = 0.37
For th given reaction,
2CH4(g) <==> C2H2(g) + 3H2(g)
Q = [C2H2][H2]^3/[CH4]^2
feeding the given values,
Q = (4.05/5.60)(10.60/5.60)^3/(6.30/5.60)^2
= 3.90
With K = 0.154,
Q > K, that is the net reaction occuring would be to the left hand side
For the given reaction,
equilibrium constant K = 0.154
When the given concentrations of reactants are added, the net reaction that would occur would be,
The reaction will proceed to the left to establish equilibrium.
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