Question

USC LILILILULLS TO ACCESS POILUL ULSII CLULU 101 LS yulJUIOL. Consider the following system at equilibrium where AH° = -111 kJ, and K = 0.159, at 723 K. N2(g) + 3H2(g) 22NH3(g) When 0.38 moles of H2(g) are added to the equilibrium system at constant temperature: The value of Kc The value of Qc Kc The reaction must run in the forward direction to restablish equilibrium. run in the reverse direction to restablish equilibrium. remain the same. It is already at equilibrium. The concentration of N, will

Answer 1

1)
Since temperature is constant, the value of Kc will be constant
Answer: do not change

2)
Qc = [product]/[reactant]
Since we are adding reactant, Qc will decrease and it will become less than Kc
Answer: less

3)
Since Qc is less than Kc, the reaction must run in forward direction to achieve equilibrium
Answer: option 1

4)
Since reaction runs in forward direction, concentration of N2 will decrease as N2 is reactant.
Answer: decrease