At 625 K the value of Kc for the equilibrium represented by the balanced equation is 2.50 x 100. Calculate the value of Kp at the same temperature. Express answer in scientific notation.
2NH3(g) = N2(g)+3H2(g)
Kp = KcRT(delta n) where delta n = n(gas products) - n(gas reactants)
whats is the boiling point of a solution composed of 17.6g of urea in (NH2)2CO in .300 kg of water
To calculate the value of Kp at the same temperature, we need to know the relationship between Kp and Kc for the given equilibrium reaction. The equation to convert between Kp and Kc is as follows:
Kp = Kc * (RT)^Δn
In this equation, 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, and Kp and Kc are the equilibrium constants in terms of pressure and concentration, respectively.
Let's look at the given balanced equation:
2NH3(g) ⇌ N2(g) + 3H2(g)
From the balanced equation, we can determine the change in the number of moles of gas:
Δn = (moles of products) - (moles of reactants) = (1+3) - 2 = 2
Now, we need to convert the temperature from °C to Kelvin. The given temperature is 625 K, which is already in Kelvin, so no conversion is needed.
Next, we substitute the values into the equation:
Kp = Kc * (RT)^Δn
Kp = (2.50 * 100) * (0.0821 * 625)^2
Now, let's calculate this value:
Kp = 250 * (0.0821 * 625)^2
Kp ≈ 250 * (0.0821 * 625)^2 = 250 * (32.256)^2
Calculating the value in scientific notation, we get:
Kp ≈ 250 * 1040.6
Kp ≈ 260,150
So, the value of Kp at the same temperature is approximately 2.6015 x 10^5 (in scientific notation).