consider the reaction:

CO (aq) + Cl2 (aq) --> COCL2 (aq).

Calculate Delta G at non standard conditions for the reaction at 298.15k, if the concentration of COCl2 is reduced to 0.01832M, while the concentrations of CO and cl2 remain at 1M. Delta G rxn = -67.4kj.

To calculate the change in Gibbs Free Energy (ΔG) at non-standard conditions for the given reaction, we can utilize the following formula:

ΔG = ΔG° + RT ln(Q)

Where:
ΔG = Change in Gibbs Free Energy
ΔG° = Standard Gibbs Free Energy Change
R = Gas constant (8.314 J/(mol·K))
T = Temperature in Kelvin
ln = Natural logarithm
Q = Reaction Quotient

Given:
ΔG° = -67.4 kJ
Temperature (T) = 298.15 K
CO concentration = 1 M
Cl2 concentration = 1 M
COCl2 concentration = 0.01832 M

First, we need to calculate the reaction quotient (Q). The reaction quotient is calculated similarly to the equilibrium constant (K), but using the concentrations of the reactants and products at non-equilibrium conditions.

Q = [COCl2] / ([CO] * [Cl2])

Substituting the given values:
Q = 0.01832 / (1 * 1) = 0.01832

Now, we can substitute the values of ΔG°, R, T, and ln(Q) into the ΔG equation to calculate ΔG:

ΔG = -67.4 kJ + (8.314 J/(mol·K) * 298.15 K * ln(0.01832))

Performing the calculation:

ΔG = -67.4 kJ + (8.314 J/(mol·K) * 298.15 K * ln(0.01832))
ΔG ≈ -67.4 kJ + (8.314 J/(mol·K) * 298.15 K * (-4.018))

Converting kJ to J:

ΔG ≈ -67,400 J + (8.314 J/(mol·K) * 298.15 K * (-4.018))

Calculating:

ΔG ≈ -67,400 J + (-9994.4 J)
ΔG ≈ -77,394.4 J

Therefore, at non-standard conditions with a COCl2 concentration of 0.01832 M while CO and Cl2 concentrations remain at 1 M, the ΔG value is approximately -77,394.4 J.

To calculate the change in Gibbs free energy (ΔG) at non-standard conditions, you can use the equation:

ΔG = ΔG° + RTln(Q)

Where:
- ΔG is the change in Gibbs free energy
- ΔG° is the standard Gibbs free energy change
- R is the gas constant (8.314 J/(mol·K))
- T is the temperature in Kelvin
- Q is the reaction quotient

In this case, you have the value of ΔG° (-67.4 kJ) and the concentrations of CO (1 M), Cl2 (1 M), and COCl2 (0.01832 M) at non-standard conditions.

First, convert the temperature to Kelvin:
T = 298.15 K

Next, we need to calculate the reaction quotient (Q). The reaction quotient is calculated using the concentrations of the reactants and products raised to the power of their respective stoichiometric coefficients.

Q = [COCl2] / ([CO] * [Cl2])

Q = (0.01832 M) / [(1 M) * (1 M)]
Q = 0.01832

Now that we have the value of Q, we can calculate the change in Gibbs free energy (ΔG) using the equation mentioned earlier:

ΔG = ΔG° + RTln(Q)
ΔG = (-67,400 J) + (8.314 J/(mol·K) * (298.15 K) * ln(0.01832)

Please note that the ln function refers to the natural logarithm.

By substituting the given values into the equation and performing the calculation, you will find the value of ΔG at non-standard conditions.