for the reaction 3C2H2=> C6H6 at 25 C, the standard enthalpy change is -631 KJ and the standard entropy change is -430 J/K. calculate the standard free energy change at 25 C. show all work!
d = delta
dGo = dHo -TdSo
To calculate the standard free energy change (∆G°) at 25°C, we can use the equation:
∆G° = ∆H° - T∆S°
Where:
∆H° = Standard enthalpy change
∆S° = Standard entropy change
T = Temperature in Kelvin
Given:
∆H° = -631 kJ
∆S° = -430 J/K
T = 25°C = 298 K
First, we need to convert ∆H° from kJ to J:
∆H° = -631 kJ = -631,000 J
Now, we can substitute the values into the equation:
∆G° = -631,000 J - (298 K)(-430 J/K)
Next, perform the multiplication:
∆G° = -631,000 J + 128,740 J
Finally, perform the addition:
∆G° = -502,260 J
Therefore, the standard free energy change (∆G°) at 25°C is approximately -502,260 J.
To calculate the standard free energy change (ΔG°) at 25°C, we can use the equation:
ΔG° = ΔH° - TΔS°
Where:
ΔH° is the standard enthalpy change (-631 kJ),
ΔS° is the standard entropy change (-430 J/K),
T is the temperature in Kelvin (25°C + 273.15 = 298.15 K).
Let's substitute the values into the equation:
ΔG° = (-631 kJ) - (298.15 K)(-430 J/K)
Now, let's convert kJ to J:
ΔG° = (-631,000 J) - (298.15 K)(-430 J/K)
Calculating the product:
ΔG° = -631,000 J + (298.15 K)(430 J/K)
Now, calculate the multiplication:
ΔG° = -631,000 J + 128,577.5 J
Adding the values together:
ΔG° = -502,422.5 J
The standard free energy change at 25°C is approximately -502,422.5 J.