Final answer:
The standard free energy change (ΔG) for a particular reaction can be calculated using the equation ΔG = ΔG° + RT ln(Q). To find ΔG at a temperature of 1.8 degrees Celsius, we need to calculate the reaction quotient (Q) using the equation Q = K × (T/298)^(Δn). Once we have Q, we can substitute it into the equation for ΔG to find ΔG at the given temperature.
Step-by-step explanation:
The standard free energy change (ΔG) for a particular reaction can be calculated using the equation ΔG = ΔG° + RT ln(Q), where ΔG° is the standard free energy change at standard conditions, R is the gas constant, T is the temperature in Kelvin, and Q is the reaction quotient. In this case, we are given ΔG° = -1332.30 kJ and ΔS = 132.80 J/K. We can calculate the reaction quotient (Q) using the equation Q = K × (T/298)^(Δn), where K is the equilibrium constant, T is the temperature in Kelvin, Δn is the change in moles of gas, and 298 is the standard temperature in Kelvin. Once we have Q, we can substitute it into the equation for ΔG to find ΔG at a temperature of 1.8 degrees Celsius.
First, we need to calculate the equilibrium constant (K). To do this, we can use the equation ΔG° = -RT ln(K).
Using the given values, we can calculate K = 5.9 × 10^(-3).
Now, we can calculate Q = K × (T/298)^(Δn). Since Δn is not given, we assume it to be zero for simplicity. Therefore, Q = K × (T/298)^0 = K.
Finally, we can substitute Q and the given values into the equation ΔG = ΔG° + RT ln(Q) to find ΔG at 1.8 degrees Celsius.
If we assume the given values are in kilojoules and joules, we will need to convert them to the same units. The given ΔG° is -1332.30 kJ, so we need to convert it to J by multiplying by 1000. The given ΔS is 132.80 J/K. We also need to convert the temperature from 1.8 degrees Celsius to Kelvin by adding 273.15.