Consider the following system at equilibrium where H° = -111 kJ, and Kc = 0.159,
ID: 951720 • Letter: C
Question
Consider the following system at equilibrium where H° = -111 kJ, and Kc = 0.159, at 723 K. N2(g) + 3H2(g) 2NH3(g)
If the VOLUME of the equilibrium system is suddenly increased at constant temperature:
The value of Kc:
A. increases. B. decreases. C. remains the same.
The value of Qc:
A. is greater than Kc. B. is equal to Kc. C. is less than Kc.
The reaction must:
A. run in the forward direction to reestablish equilibrium. B. run in the reverse direction to reestablish equilibrium. C. remain the same. It is already at equilibrium.
The number of moles of H2 will:
A. increase. B. decrease. C. remain the same.
Explanation / Answer
N2(g) + 3H2(g) ------------------> 2NH3(g)
If the VOLUME of the equilibrium system is suddenly increased at constant temperature ten pressure of the system will decrease. then reaction proceed to increase the pressure by producing more number of moles (toeatds reactants).
The value of Kc remains the same
The value of Qc is greater than Kc
The reaction must run in the reverse direction to reestablish equilibrium
The number of moles of H2 will increase