Question

The gas-phase reaction of H2 with CO2 to produce H2O and CO has ΔH=11kJ and ΔS=41J/K. Is the reaction spontaneous at 298.15 K? What is ΔG?

a) The reaction is spontaneous; ΔG=−11kJ.
b) The reaction is not spontaneous; ΔG=11kJ.
c) The reaction is spontaneous; ΔG=11kJ.
d) The reaction is not spontaneous; ΔG=−11kJ.

Answer 1

The reaction of H2 with CO2 to produce H2O and CO is spontaneous at 298.15 K according to the Gibbs free energy change calculation.

Step-by-step explanation:

The reaction of H2 with CO2 to produce H2O and CO is spontaneous at 298.15 K. This can be determined by calculating the Gibbs free energy change (ΔG) using the equation ΔG = ΔH - TΔS, where ΔH is the enthalpy change, ΔS is the entropy change, and T is the temperature in Kelvin.

In this case, ΔH = 11 kJ and ΔS = 41 J/K. Plugging these values into the equation, we get ΔG = 11 kJ - (298.15 K × 41 J/K).

Solving this equation, we find that ΔG = -9.6 kJ. Since ΔG is negative, the reaction is spontaneous.