Answer :
Answer:
- a) Q > K and more reactants will be made to reach equilibrium
Explanation:
The reaction quotient, Q, is the actual ratio of concentrations or pressure of products to reactants.
When Q is equal to the equilibrium constant, the reaction is at equilibrium.
When Q > K, the concentrations, or pressures, of the products will have to decrease to reach the equilibrium, thus more reactants will be made.
When Q < K the concentrations, or pressures, of the reactants will have to decrease to reach the equilibrium, thus more products will be made.
Calculate Q:
- Reaction equation: Cl₂(g) + Br₂(g) ⇄ 2 BrCl(g),
[tex]P_{Cl_2}}=0.19bar\\\\P_{Br_2}}=0.29bar\\\\P_{BrCl}=1.4bar[/tex]
[tex]Q=\dfrac{(P_{BrCl})^2}{(P_{Br_2}).(P_{Cl_2})}[/tex]
[tex]Q=\dfrac{(1.4bar)^2}{(0.19bar).(0.29bar)}[/tex]
[tex]Q\approx 36[/tex]
Therefore, since Q > K, the pressure of the products should decrease to reach the equilibrium, meaning that more reactants will be made, i.e. option a).
The mixture is analyzed and found to contain 0.19 bar of Cl2, 0.29 bar of Br2 and 1.4 bar of BrCl, the situation will be Q > K and more reactants will be made to reach equilibrium.
What is gas-phase reaction?
The reaction occur in gas phase are called gas phase reaction.
Given reaction is
[tex]\rm Cl_2(g) + Br_2(g) <=> 2 BrCl(g)[/tex]
[tex]Cl_2 = 0.19\; bar\\\\Br_2=0.29 \;bar\\\\BrCl = 1.4\;bar[/tex]
Calculating the value of Q
[tex]Q = \dfrac{(P_B_r_C_l)^2}{(P_B_r_2)(P_C_l_2)} \\\\Q =\dfrac{(1.4\;bar)^2}{(0.29\;bar)( 1.9\;bar)}\\\\Q= 36[/tex]
Thus, the correct option is (a), Q > K and more reactants will be made to reach equilibrium.
Learn more about gas phase, here:
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