At 1100 K, Kp = 0.25 for the following reaction.
2 SO2(g) + O2(g) 2 SO3(g)
What is the value of K at this temperature?
To find the value of K at a given temperature, we can use the relationship between Kp and K. The relationship between Kp and K is given by the following equation:
Kp = K(RT)^(∆n)
Where:
- Kp is the equilibrium constant in terms of partial pressures.
- K is the equilibrium constant in terms of concentration.
- R is the gas constant (0.0821 L·atm/mol·K).
- T is the temperature in Kelvin.
- ∆n is the change in the number of moles of gas particles in the balanced chemical equation.
In the given reaction:
2 SO2(g) + O2(g) → 2 SO3(g)
The change in the number of moles of gas particles (∆n) is equal to the sum of the coefficients of the product gases minus the sum of the coefficients of the reactant gases:
∆n = (2 + 0) - (2 + 1) = 3 - 3 = 0
Since ∆n is zero, it means that Kp and K are equal. Therefore, the value of K at this temperature (1100 K) is also 0.25.
To find the value of K at a given temperature, we can use the equation:
K = Kp(RT)^(Δn)
Where K is the equilibrium constant, Kp is the equilibrium constant expressed in terms of partial pressures, R is the gas constant (8.314 J/(mol·K)), T is the temperature in Kelvin, and Δn is the change in the number of moles of gas from the reactants to the products.
In this case, we are given Kp = 0.25 and the equation for the reaction is:
2 SO2(g) + O2(g) -> 2 SO3(g)
So, based on the coefficients of the balanced equation, the change in the number of moles of gas is Δn = (2+1) - (2) = 1.
Now, we need to convert the temperature to Kelvin. If the given temperature is in Celsius, we can add 273.15 to convert it to Kelvin. Let's assume the temperature is already in Kelvin.
Substituting the given values into the equation, we have:
K = 0.25 * (8.314 J/(mol·K)) * (1100 K)^1
Calculating this expression gives us the value of K at this temperature.
Do you want Kc? That is
Kp = Kc(RT)^delta n.
Substitute and solve for Kc.