At 1500 °C, Kc = 5.67 for the reaction
CH4(g) + H2O(g) CO(g) + 3H2(g)
Calculated value of ΔG°1773 for the reaction at this temperature.
The answer is -174 kJ
To calculate the standard Gibbs free energy change (ΔG°) for the reaction at this temperature, you can use the equation:
ΔG° = -RT ln(K)
Where:
ΔG°: Standard Gibbs free energy change
R: Gas constant (8.314 J/(mol⋅K))
T: Temperature in Kelvin (1500 °C = 1773 K)
K: Equilibrium constant (Kc = 5.67)
Now, let's plug in the values and calculate ΔG°:
ΔG° = - (8.314 J/(mol⋅K)) × 1773 K × ln(5.67)
Calculating this expression gives us the value of ΔG°1773 for the reaction.
To calculate the value of ΔG° (standard Gibbs free energy change) for the reaction at 1500 °C (1773 K), you will need the equation:
ΔG° = -RT ln K
Where:
ΔG° is the standard Gibbs free energy change
R is the gas constant (8.314 J/(mol∙K))
T is the temperature in Kelvin
K is the equilibrium constant (Kc in this case)
First, convert the given temperature from Celsius to Kelvin by adding 273:
T = 1500 °C + 273 = 1773 K
Next, substitute the values into the equation:
ΔG° = - (8.314 J/(mol∙K)) * (1773 K) * ln 5.67
To calculate ln (natural logarithm), you can use a scientific calculator or an online calculator. Simply input the value 5.67 and press the ln button. The result should be a negative number.
Finally, multiply the calculated value of -RT ln K to get the value of ΔG° for the reaction at 1500 °C.
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