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Nitrogen and oxygen gases may react to form nitrogen monoxide. At 1500 °C, Kc equals 1.0 × 10−5.   N2(g) + O2(g) 2 NO(g)   If 0.030 mol N2 and 0.030 mol O2 are sealed in a 1.0 L flask at 1500 °C, what is the concentration of NO(g) when equilibrium is established?

Write a balanced chemical equation which corresponds to the following equilibrium constant expression.

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?

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

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).

A student analyzed a first-order reaction and obtained the graph below. Unfortunately, the student forgot to label the axes. What are the correct labels for the x and y axes?

A mixture of nitrogen and hydrogen was allowed to come to equilibrium at a given temperature. 3H2 + N2    2NH3 An analysis of the mixture at equilibrium revealed 2.1 mol N2, 2.8 mol H2, and 1.8 mol NH3. How many moles of H2 were present at the beginning of the reaction?

The Arrhenius equation, expresses the dependence of the rate constant on the reaction temperature. The slope of a plot of ln(k) versus 1/T is equal to

Which of the following statements is/are CORRECT?   1. For a chemical system, if the reaction quotient (Q) is greater than K, reactant must be converted to products to reach equilibrium.   2. For a chemical system at equilibrium, the forward and reverse rates of reaction are equal.   3. For a chemical system at equilibrium, the concentrations of products divided by the concentrations of reactants equals one.

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