Use the reaction I2(s) I2(g), H = 62.4 kJ/mol, S = 0.145 kJ/(molK), for this question.Which direction of the reaction is favored at 298 K (room temperature)?A.Toward I2(s) productionB.It is impossible to tell.C.Toward I2(g) productionD.Both are equally favored.SUBMITarrow_backPREVIOUS

To determine the direction of the reaction that is favored at a given temperature, we can use the Gibbs free energy equation:

ΔG = ΔH - TΔS

where: ΔG is the change in Gibbs free energy, ΔH is the change in enthalpy (62.4 kJ/mol in this case), T is the absolute temperature in Kelvin (298 K in this case), and ΔS is the change in entropy (0.145 kJ/(molK) in this case).

First, convert ΔH and ΔS to the same units. Since ΔS is in kJ/(molK), convert ΔH to kJ by multiplying by 1,000:

ΔH = 62.4 kJ/mol = 62,400 J/mol

Now, substitute the given values into the Gibbs free energy equation:

ΔG = 62,400 J/mol - (298 K * 0.145 kJ/(molK) * 1,000 J/kJ) ΔG = 62,400 J/mol - 43,210 J/mol ΔG = 19,190 J/mol

Since ΔG is positive, the reaction is not spontaneous in the direction written. Therefore, the reaction is favored in the opposite direction, toward I2(s) production. So, the answer is A. Toward I2(s) production.

To determine the direction of the reaction that is favored at a given temperature, we can use the Gibbs free energy equation:

ΔG = ΔH - TΔS

where: ΔG is the change in Gibbs free energy, ΔH is the change in enthalpy (heat content), T is the absolute temperature in Kelvin, and ΔS is the change in entropy (disorder).

Given in the problem, we have ΔH = 62.4 kJ/mol and ΔS = 0.145 kJ/(molK). The temperature T is 298 K.

First, convert ΔH and ΔS to the same units. Here, ΔH is in kJ/mol and ΔS is in kJ/(molK), so they are already in the same units.

Now, substitute the given values into the Gibbs free energy equation:

ΔG = 62.4 kJ/mol - (298 K * 0.145 kJ/(molK))

Calculate the value of ΔG. If ΔG is negative, the reaction is spontaneous and proceeds in the forward direction (toward I2(g) production). If ΔG is positive, the reaction is non-spontaneous and proceeds in the reverse direction (toward I2(s) production). If ΔG is zero, both directions are equally favored.