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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()

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

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)

At 800 K, the equilibrium constant, Kp, for the following reaction is 3.2 × 10–7. 2 H2S(g) 2 H2(g) + S2(g) A reaction vessel at 800 K initially contains 3.00 atm of H2S. If the reaction is allowed to equilibrate, what is the equilibrium pressure of S2?

Which of the following statements is true if reaction quotient (Q) is greater than equilibrium constant (K)?

For a certain reaction of the general form aA → products, a plot of the experimental data of ln[A] versus time is linear. What is the reaction order with respect to the reactant (A)?

Below is a proposed mechanism for the decomposition of H2O2. H2O2 + I– → H2O + IO– slow H2O2 + IO– → H2O + O2 + I– fast Which of the following statements is incorrect?