Question

To the first decimal place, what is Delta G in kJ for a chemical reaction at 24.4°C where Delta S is 20.79 J/mol-K and Delta H is-39.5 kJ?

Answer 1

Step-by-step explanation:

To calculate Delta G in kJ for a chemical reaction at 24.4°C, we can use the equation:

Delta G = Delta H - T * Delta S

where Delta H is the enthalpy change in kJ/mol, Delta S is the entropy change in J/mol-K, T is the temperature in Kelvin, and Delta G is the free energy change in kJ/mol.

First, we need to convert the temperature to Kelvin:

T = 24.4°C + 273.15 = 297.55 K

Next, we can substitute the given values into the equation:

Delta G = -39.5 kJ/mol - (297.55 K) * (20.79 J/mol-K / 1000 J/kJ)

Delta G = -39.5 kJ/mol - 6.18 kJ/mol

Delta G = -45.68 kJ/mol

Rounding to the first decimal place, we get Delta G = -45.7 kJ/mol.

Answer 2

Step-by-step explanation:

To calculate Delta G in kJ for a chemical reaction at 24.4°C where Delta S is 20.79 J/mol-K and Delta H is -39.5 kJ, we can use the equation:

ΔG = ΔH - TΔS

where ΔH is the enthalpy change, ΔS is the entropy change, T is the temperature in Kelvin, and ΔG is the Gibbs free energy change.

First, we need to convert the temperature from Celsius to Kelvin:

T = 24.4°C + 273.15 = 297.55 K

Next, we can plug in the values for ΔH, ΔS, and T:

ΔG = -39.5 kJ - (297.55 K)(20.79 J/mol-K / 1000) = -44.6 kJ

Rounding to the first decimal place, the value of ΔG is -44.6 kJ.

Therefore, the answer is -44.6 kJ.