Determine ΔG°rxn using the following information. H2(g) + CO(g) → CH2O(g)   ΔH°= +1.9 kJ ΔS°= -109.6 J/K

The equilibrium constant is given for one of the reactions below. Determine the value of the missing equilibrium constant.         2 SO2(g) + O2(g) ⇌ 2 SO3(g)           Kc = 1.7 × 106        SO3(g) ⇌ 1/2 O2(g) + SO2(g)           Kc = ?

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          2 HBr(g) ⇌ H2(g) + Br2(g)    Kc = ?

The following reaction is endothermic. What effect will decreasing the temperature have on the system?                           I2(g) + Cl2(g) ⇌ 2 ICl(g)

Place the following in order of increasing standard molar entropy.

Determine ΔG°rxn using the following information. 2 H2S(g) + 3 O2(g) → 2 H2O(l) + 2 SO2(g) ΔH°= +1.12 kJ ΔS°= -390.7 J/K

Consider the following reaction at equilibrium. What effect will adding more SO3 have on the system?              SO2(g) + NO2(g) ⇌ SO3(g) + NO(g)

Calculate ΔS°rxn for the following reaction. The S° for each species is shown below the reaction.                        N2H4(l) + H2(g) → 2 NH3(g)  S° (J/mol∙K)  121.2       130.7         192.8

The first-order rearrangement of CH3NC is measured to have a rate constant of 3.61 × 10-15 s-1 at 298 K and a rate constant of 8.66 × 10-7 s-1 at 425 K. Determine the activation energy for this reaction.

Chemical equilibrium is the result of _______