Calculate Kp for the reaction N2(g) + 3 H2(g)--> 2 NH3(g) given that the reaction has Kc = 438,880,639 at a temperature of 265.
To calculate Kp for the given reaction, you need to know Kc, the equilibrium constant, as well as the gas constant, R, and the temperature, T.
The given Kc is 438,880,639 at a temperature of 265. However, Kp and Kc are related by the equation:
Kp = Kc * (RT)^(∆n)
Where:
Kp is the equilibrium constant in terms of partial pressures,
Kc is the equilibrium constant in terms of concentrations,
R is the ideal gas constant (0.0821 L.atm/(mol.K)),
T is the temperature in Kelvin,
∆n is the change in moles of gas between the products and reactants.
In the given reaction, N2(g) + 3 H2(g) --> 2 NH3(g), there is a decrease in the number of moles of gas as the reaction proceeds (∆n = 2 - (1 + 3) = -2).
Now, we can calculate Kp using the given Kc value, R, and T.
Kp = Kc * (RT)^(∆n)
= 438,880,639 * (0.0821)^(2) * (265)^(-2)
= 438,880,639 * 0.006775 * 0.01512
≈ 4.487
Therefore, Kp for the reaction N2(g) + 3 H2(g) --> 2 NH3(g) at a temperature of 265 is approximately 4.487.
To calculate Kp, we need to know the relationship between Kp and Kc.
For the given reaction: N2(g) + 3 H2(g) --> 2 NH3(g)
The relationship is: Kp = Kc(RT)^(Δn)
Where:
- Kp is the equilibrium constant in terms of partial pressures
- Kc is the equilibrium constant in terms of molar concentrations
- R is the ideal gas constant (0.0821 L·atm/(mol·K))
- T is the temperature in Kelvin
- Δn is the change in the number of moles of gas from reactants to products
In this reaction:
- Δn = (2 + 0) - (1 + 3) = -2
Given: Kc = 438,880,639
T = 265 K
Now, we can calculate Kp.
Kp = Kc(RT)^(Δn)
Kp = 438,880,639 * (0.0821 L·atm/(mol·K))^(-2) * 265 K
Let's calculate the value of Kp using these values:
Kp = 438880639 * (0.0821)^(-2) * 265 = 1.34 x 10^6
Therefore, Kp for the reaction N2(g) + 3 H2(g) --> 2 NH3(g) is approximately 1.34 x 10^6.