Assume that the following endothermic chemical reaction is at equilibrium. C(s) + H2O(g) H2(g) + CO(g) Which of the following statements is/are CORRECT?   1. Increasing the concentration of H2(g) will cause the reaction to proceed in the backward direction, increasing the equilibrium concentration of H2O(g).   2. Decreasing the temperature will cause the reaction to proceed in the forward direction, increasing the equilibrium concentration of CO(g).   3. Increasing the amount of C(s) will cause the reaction to proceed in the forward direction, increasing the equilibrium concentration of CO(g).

For the reaction provided, the rate of disappearance of IO3–(aq) at a particular time and concentration is 2.6 × 10-3 mol/L·s. IO3–(aq) + 5I–(aq) + 6H+(aq) → 3I2(aq) + 3H2O(l) What is the relative rate of appearance of I2(aq)?

A 2.5 L flask is filled with 0.25 mol SO3, 0.20 mol SO2, and 0.40 mol O2, and allowed to reach equilibrium. Assume the temperature of the mixture is chosen so that Kc = 0.12. Predict the effect on the concentration of SO3 as equilibrium is achieved by using Q, the reaction quotient. 2 SO3(g) 2 SO2(g) + O2(g)

A 3.00-liter flask initially contains 3.00 mol of gas A and 1.50 mol of gas B. Gas A decomposes according to the following reaction: 3A  2B + C The equilibrium concentration of gas C is 0.134 mol/L. Determine the value of the equilibrium constant, Kc.

For the equilibrium PCl5(g) PCl3(g) + Cl2(g), Kc = 4.0 at 228°C. If pure PCl5 is placed in a 1.00-L container and allowed to come to equilibrium, and the equilibrium concentration of PCl5(g) is 0.19 M, what is the equilibrium concentration of PCl3?

Molecules must overcome a barrier called the activation energy if they are to react. The highest energy point reached during the progress of a reaction is called the ____.

The following data were obtained in a kinetics study of the hypothetical reaction A + B + C → products. [A]0 (M) [B]0 (M) [C]0 (M) Initial Rate (10–3 M/s) 0.4 0.4 0.2 160 0.2 0.4 0.4 80 0.6 0.1 0.2 15 0.2 0.1 0.2 5 0.2 0.2 0.4 20 What is the order of the reaction with respect to C?

Consider the reaction below. 2 HF(g) H2(g) + F2(g) (Kc = 1.00 × 10–2) Given that 1.00 mol of HF(g), 0.241 mol of H2(g), and 0.750 mol of F2(g) are mixed in a 5.00 L flask, determine the reaction quotient, Q.

Given the following chemical equilibria,   N2(g) + O2(g) 2 NO(g) K1   N2(g) + 3 H2(g) 2 NH3(g) K2   H2(g) + 1/2 O2(g) H2O(g) K3 Determine the method used to calculate the equilibrium constant for the reaction below.   4 NH3(g) + 5 O2(g) 4 NO(g) + 6 H2O(g) K c

Write the expression for Kp for the reaction below. 2 NOBr(g) 2 NO(g) + Br2()