for the reaction 1/2 F2(g) = F(g) a reaction mixture initially contains ).5atm of F2(g) and 0.5 atm of F(g) in their standard states. If Kp = 7.55x10-2 at this temperature which statement is true? a. Q>K and the reaction proceeds towards the reactants b. Q

10 For a chemical reaction: Cl2 (1) 0.55 mol Cl₂ Solve for the final partial pressure of Cl in atm: A. 1.8 × 108 B. 8.9 x 105 D. 3.6 × 104 2 Cl (g) has a Kp =3.2 x 10", and the initial amounts are: 0 atm Cl E. 0.55 C. 1.8 104 10.8

Consider the following system at equilibrium where H° = -111 kJ/mol, and Kc = 0.159, at 723 K. N2(g) + 3H2(g) 2NH3(g) If the TEMPERATURE on the equilibrium system is suddenly decreased: The value of Kc fill in the blank 1 A. increases.     B. decreases.     C. remains the same.   The value of Q fill in the blank 2 A. is greater than Kc.     B. is equal to Kc.     C. is less than Kc.   The reaction must: fill in the blank 3 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 concentration of H2 will: fill in the blank 4 A. increase.     B. decrease.     C. remain the same.

Consider the following reaction: 2 CO2 (g) + 2 H, = 2 CO (g) + 2 H20 (g) K= 6.00 At the start of the reaction, the flask contains 0.550 atm CO2, 0.300 atm H2, and 1.20 atm CO, and 1.50 atm H20. a. Calculate the value of the reaction quotient, Q. b. Which direction will the reaction proceed to achieve equilibrium?