The equilibrium constant is given for one of the reactions below. Determine the value of the missing equilibrium constant. H2(g) + Br2(g) ⇌ 2 HBr(g)            Kc = 3.8 × 104 4 HBr(g) ⇌ 2 H2(g) + 2 Br2(g)      Kc = ?

Which of the changes listed will shift the equilibrium to the right for the following reversible reaction? CH4(g) + H2O(g) + heat CO(g) + 3 H2(g)

For the reaction:  I2 (g) ⇌ 2 I (g) at 1000 K, the value of Kc = 3.76 × 10-5. A 2.00-L flask initially contains 1.00 mole of I2 and no iodine atoms is heated. After the system reaches equilibrium, what are the equilibrium concentrations of I2 and I? Hint: Use an ICE table (Initial, Change, Equilibrium) to express each concentration in terms of x.

The equilibrium constant expression for the reaction: 2 BrF5(g) ⇌ Br2(g) + 5 F2(g) is

The reaction below has a Kp value of 3.30 × 10-5. What is the value of Kc for this reaction at 700. K? 2 SO3(g) ⇌ 2 SO2(g)  + O2(g)

The following is an Arrhenius plot of a first-order reaction. The rate constant is measured in units of s–1.   Based on this Arrhenius plot, what is the activation energy (Ea) of the reaction? Hint: Use the Arrhenius linear form shown below to determine the activation energy (Ea). Match the graph to the equation:  R is the gas constant (8.314 J/mol . K)

Consider the following reaction at equilibrium. What effect will reducing the pressure of the reaction mixture have on the system? Xe(g) + 2 F2(g) ⇌ XeF4(g)

A first-order reaction has a rate constant (k) of 0.241/ min. If the initial concentration of A is 0.859 M, what is the concentration of A after 10.0 minutes?

Which of the following best describes the concept of risk aversion?

Which actions by the unit manager best reflect organizational ethics and a culture of safety? (Select all that apply.)