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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