Consider the following reaction (assume an ideal gas midure): 2NOBr( g) 2NO 9) + Br 2( g) A10-ter vessel was initially filled with pure NOBr, at a pressure of 4.0 atm, at 300 K. After equilibrium was established, the partial pressure of NOBr was 3 1 atm. What is K for the reaction? OA0 26 OB0 13 OCD 038 OD0 45 OE none of these

1. The diagrams below represent the following reversible chemical reaction: H2(g) + 12 (g) =2 HI (g) At 448 °C, the equilibrium constant, K, for this reaction is 51 Initial Conditions: Temperature = 448 °C Volume of the container = 2.0 L 0 = 1 mole H2 (g) = 1 mole I2 (g) 00 00 .. 00 00 •. What is the initial molar concentration of hydrogen. [H:]? What is the initial molar concentration of iodide, [I2]? M This system will reach equilibrium when rate of the forward reaction is equal to the rate of the reverse reaction. Write the equilibrium constant expression, Kc, for this reaction: Calculate the equilibrium concentrations for H;(g), I (g) and HI (g) H2(g}_ + l2 (g) 2 HI (g) [H2] [L2] [HI Initial Change Equilibrium +2x -X-

For the reaction H2(g) + Br2(g) =2 HBr(g), Kc = 81.4 at 385°C. If [H2] = [Br2] = [HBr] = 2.4 x 10-4 M at 385°C, which one of the following is correct? %3D [HBr] increases as the system approaches equilibrium. [H2] and [HBr] decreases as the system moves toward equilibrium. [H2] and [Br2] increases as the system approaches equilibrium. There is not enough information given to make a determination. [HBr] and [Br2] increases as the system approaches equilibrium. The system is at equilibrium.

0.31 M of F₂ gas and excess solid of E were placed in a container. When the following reaction has reached equilibrium, the concentration of EF gas was 0.024 M. What is the equilibrium concentration of F₂ gas? Please report 3 decimal places, without units. 2E(s) + F₂(g) →→→ 2EF(g)