H° = 565 kJ and S° = -11.1 J/K
Calculate G° at 25°C for this reaction.
Use the Gibbs Free Energy Equation:
^G=^H-T^S
;where ^ represents Delta.
Plug in the values and you are done!
Remember to convert 25C to Kelvin.
To calculate the standard Gibbs free energy (ΔG°) at 25°C for a reaction, we can use the equation:
ΔG° = ΔH° - TΔS°
where:
- ΔH° is the standard enthalpy change
- ΔS° is the standard entropy change
- T is the temperature in Kelvin (25°C is 298 K)
Given:
ΔH° = 565 kJ
ΔS° = -11.1 J/K
T = 298 K
Let's plug in the values and calculate ΔG°:
ΔG° = 565 kJ - (298 K) * (-11.1 J/K)
First, we need to convert kJ to J:
ΔG° = 565,000 J - (298 K) * (-11.1 J/K)
Next, we multiply the temperature term:
ΔG° = 565,000 J + 3,308 J
Finally, we calculate the sum:
ΔG° = 568,308 J
Therefore, the standard Gibbs free energy (ΔG°) at 25°C for this reaction is approximately 568,308 J.
To calculate the standard Gibbs free energy change (ΔG°) at 25°C for a reaction, you can use the equation:
ΔG° = ΔH° - TΔS°
where ΔH° is the standard enthalpy change, ΔS° is the standard entropy change, and T is the temperature in Kelvin.
Given:
ΔH° = 565 kJ (convert to J by multiplying by 1000)
ΔS° = -11.1 J/K
T = 25°C = 298 K (convert to Kelvin by adding 273)
First, convert the units of ΔH°:
ΔH° = 565 kJ * 1000 = 565,000 J
Next, substitute the values into the equation:
ΔG° = 565,000 J - (298 K * -11.1 J/K)
To simplify, multiply the temperature and ΔS°:
ΔG° = 565,000 J + (298 K * 11.1 J)
Finally, calculate the value of ΔG°:
ΔG° = 565,000 J + 3,303 J
ΔG° = 568,303 J
Therefore, the standard Gibbs free energy change (ΔG°) at 25°C for this reaction is 568,303 J.