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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?

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

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?

Given the following chemical equilibrium COCl2(g)  CO(g) + Cl2(g), calculate the value of Kc when Kp = 6.5 × 1011 at 298 K. (R = 0.08206 L⋅atm/mol ⋅ K)

What is the Kc expression for the equilibrium given below? CuI(s) Cu+(aq) + I−(aq)

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

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.

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

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?

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?