QuestionMay 6, 2025

Calculate Delta G_(rxn)^circ (in kJ) for a reaction where Delta H^circ =-99kJ,Delta S^circ =+245J/K and T=298K square

Calculate Delta G_(rxn)^circ (in kJ) for a reaction where Delta H^circ =-99kJ,Delta S^circ =+245J/K and T=298K square
Calculate Delta G_(rxn)^circ (in kJ) for a reaction where Delta H^circ =-99kJ,Delta S^circ =+245J/K and T=298K square

Solution
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Answer

-171.91 \, \text{kJ} Explanation 1. Identify the formula Use the Gibbs free energy formula: **\Delta G_{rxn}^{\circ} = \Delta H^{\circ} - T\Delta S^{\circ}**. 2. Convert units Convert \Delta S^{\circ} from J/K to kJ/K: 245 \, \text{J/K} = 0.245 \, \text{kJ/K}. 3. Substitute values Substitute into the formula: \Delta G_{rxn}^{\circ} = -99 \, \text{kJ} - 298 \times 0.245 \, \text{kJ/K}. 4. Calculate Perform the calculation: \Delta G_{rxn}^{\circ} = -99 - 72.91 = -171.91 \, \text{kJ}.

Explanation

1. Identify the formula<br /> Use the Gibbs free energy formula: **$\Delta G_{rxn}^{\circ} = \Delta H^{\circ} - T\Delta S^{\circ}$**.<br /><br />2. Convert units<br /> Convert $\Delta S^{\circ}$ from J/K to kJ/K: $245 \, \text{J/K} = 0.245 \, \text{kJ/K}$.<br /><br />3. Substitute values<br /> Substitute into the formula: $\Delta G_{rxn}^{\circ} = -99 \, \text{kJ} - 298 \times 0.245 \, \text{kJ/K}$.<br /><br />4. Calculate<br /> Perform the calculation: $\Delta G_{rxn}^{\circ} = -99 - 72.91 = -171.91 \, \text{kJ}$.
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