Above what temperature does the following reaction become nonspontaneous? FeO(s) + CO(g) → CO2(g) + Fe(s)      ΔH = -11.0 kJ ΔS = -17.4 J/K

Determine the rate law and the value of k for the following reaction using the data provided. S2O82⁻(aq) + 3 I⁻(aq) → 2 SO42⁻(g) + I3⁻(aq)  [S2O82⁻]i (M)         [I⁻]i (M)         Initial Rate    0.30                      0.42                 4.54    0.44                      0.42                 6.65    0.44                      0.21                 3.33

Write a balanced reaction for which the following rate relationships are TRUE. Rate = –

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of H2O(g). C2H4(g) + H2O(g) ⇌ C2H5OH(g)   Kc = 9.0 × 103 [C2H4]eq = 0.015 M                        [C2H5OH]eq = 1.69 M

Given the following balanced equation, determine the rate of reaction with respect to [NOCl].                                               2 NO(g) + Cl2(g) → 2 NOCl(g)

Above what temperature does the following reaction become nonspontaneous? 2 H2S(g) + 3 O2(g) → 2 SO2(g) + 2 H2O(g)    ΔH = -1,036 kJ ΔS = -153.2 J/K

The following reaction is exothermic. What set of conditions will always lead to the equilibrium shifting to the left?                                    2 NO(g) + Br2(g) ⇌ 2 NOBr(g)

Determine the rate law and the value of k for the following reaction using the data provided. 2 NO(g) + O2(g) → 2 NO2(g) [NO]i (M)       [O2]i (M)      Initial Rate (1/M·s) 0.030               0.0055           8.55 × 10-3 0.030               0.0110           1.71 × 10-2 0.060               0.0055           3.42 × 10-2

Consider the following reaction at equilibrium. What effect will removing H2O have on the system?         2 H2S(g) + 3 O2(g) ⇌ 2 H2O(g) + 2 SO2(g)

Use the free energies of formation given below to calculate the equilibrium constant (K) for the following reaction at 298 K.                                              2 HNO3(aq) + NO(g) → 3 NO2(g) + H2O(l)           K = ?                ΔG°f (kJ/mol):          -110.9           87.6           51.3       -237.1