The equilibrium constant for the reaction below is 7.2 × 10-4at 298 K and 1 atm.HNO2(aq) + H2O(l) NO2-(aq) + H3O+(aq)When [HNO2(aq)] = 1.0 M and [NO2-(aq)] = [H3O+(aq)] = 1.0× 10-5 M, calculate ΔG.
Question
The equilibrium constant for the reaction below is 7.2 × 10-4at 298 K and 1 atm.HNO2(aq) + H2O(l) NO2-(aq) + H3O+(aq)When [HNO2(aq)] = 1.0 M and [NO2-(aq)] = [H3O+(aq)] = 1.0× 10-5 M, calculate ΔG.
Solution
To calculate ΔG, we can use the formula:
ΔG = -RT ln(K)
where: R is the gas constant, which is 8.314 J/(mol·K) T is the temperature in Kelvin, which is 298 K K is the equilibrium constant, which is 7.2 × 10^-4
First, we need to convert the equilibrium constant into natural logarithm form:
ln(K) = ln(7.2 × 10^-4) = -7.234
Then, we can substitute the values into the formula:
ΔG = - (8.314 J/(mol·K)) * (298 K) * (-7.234) ΔG = 17934.8 J/mol
However, the standard unit for ΔG is kJ/mol, so we need to convert J/mol to kJ/mol:
ΔG = 17934.8 J/mol * (1 kJ/1000 J) = 17.93 kJ/mol
So, the ΔG for the reaction is 17.93 kJ/mol.
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