question 18 parts a and b

Consider the following system at equilibrium where H=16.1kJ/mol, and Kc=6.50103, at 298K. 2NOBr(g)2NO(g)+Br2(g) When 0.17 moles of NOBr(g) are added to the equilibrium system at constant temperature: The value of Kc The value of QcKc. 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 NO will Consider the following system at equilibrium where H=92.7kJ, and Kc=1.80104, at 298K NH4HS(s)NH3(g)+H2S(g) When some moles of NH4HS(s) are added to the equilibrium system at constant temperature: The value of Kc increases decreases remains the same The value of Qc is greater than Kc is equal to Kc is less than Kc The reaction must run in the forward direction to reestablish equilibrium. run in the reverse direction to reestablish equilibrium. remain the same. It is already at equilibrium. The number of moles of NH3 will increase decrease remain the same