I need to find delta G but I keeo getting 8722.2...I know the formula, can someone help me? ΔH = -19.2 kJ/mol; ΔS = 261 J/mol·K; T = 315 K
I've tried, I thought, all of the combinations and I can't come up with 8722.2. It would have helped if you had put units on your answer.
DG = DH - TDS
DG = -19.2 kJ/mol -(315)(0.261 kJ/mol)
DG = -19.2 kJ/mol - 82.215 = -101.4 kJ/mol
Check my work.
Ohhh no, I see what i did, I didn't convert the J into kj...okay thank u!
I expect that is the most common student error.
To calculate the Gibbs free energy change (ΔG), you can use the equation: ΔG = ΔH - TΔS. Here, ΔH represents the enthalpy change, ΔS represents the entropy change, and T represents the temperature in Kelvin.
Given:
ΔH = -19.2 kJ/mol
ΔS = 261 J/mol·K
T = 315 K
First, let's convert ΔH to J/mol:
ΔH = -19.2 kJ/mol = -19,200 J/mol
Now, apply the values in the equation:
ΔG = ΔH - TΔS
ΔG = -19,200 J/mol - (315 K * 261 J/mol·K)
Next, calculate TΔS:
TΔS = 315 K * 261 J/mol·K = 82,215 J/mol
Substitute the value of TΔS back into the equation:
ΔG = -19,200 J/mol - 82,215 J/mol
Finally, calculate the ΔG value:
ΔG = -101,415 J/mol
So, the calculated ΔG value is -101,415 J/mol.