The thermodynamic equilibrium constant for the following reaction is 0.15 at 1227°C.
2 SO2(g) + O2(g) 2 SO3(g)
Which is true? Can be more than one answer.
a. The reaction is product-favored.
b. The reaction is reactant-favored.
c. G°is less than zero.
d. G° is greater than zero.
e. G° is equal to zero.
THANKS!
To determine the favorability of a reaction and the sign of the change in Gibbs free energy (ΔG), we need to consider the value of the equilibrium constant (K) and the temperature.
The relationship between ΔG and K is given by the equation:
ΔG° = -RT ln(K)
Where:
- ΔG° is the change in Gibbs free energy under standard conditions (standard state),
- R is the gas constant (8.314 J/(mol·K)),
- T is the temperature in Kelvin (K), and
- ln denotes the natural logarithm.
First, let's convert the temperature given in Celsius to Kelvin:
1227°C = 1499 K (approximately)
Now, we can assess the statement options:
a. The reaction is product-favored.
For a reaction to be product-favored, the equilibrium constant (K) should be greater than 1. In this case, as the equilibrium constant is 0.15, it is less than 1, so this statement is not true.
b. The reaction is reactant-favored.
For a reaction to be reactant-favored, the equilibrium constant (K) should be less than 1. In this case, as the equilibrium constant is 0.15, it is less than 1, so this statement is true.
c. G° is less than zero.
If G° is less than zero, it means that the reaction is spontaneous in the forward direction. Since the equilibrium constant is less than 1, it indicates that G° must be less than zero. Therefore, this statement is true.
d. G° is greater than zero.
If G° is greater than zero, it means that the reaction is non-spontaneous under standard conditions. Since the equilibrium constant is less than 1, it indicates that G° must be less than zero. Therefore, this statement is false.
e. G° is equal to zero.
If G° is equal to zero, it means that the reaction is at equilibrium under standard conditions. However, since the equilibrium constant is 0.15, it indicates that G° must be less than zero. Therefore, this statement is false.
In conclusion, the correct statements are:
b. The reaction is reactant-favored.
c. G° is less than zero.