The following equilibrium pressures were observed at a certain temperature for the reaction.
N2(g) + 3 H2(g) <==> 2 NH3(g)
partial pressure of NH3 = 3.2 ✕ 10−1 atm
partial pressure of N2 = 1.6 ✕ 10−2 atm
partial pressure of H2 = 4.9 ✕ 10−2 atm
Calculate the value for the equilibrium constant Kp at this temperature.
i got 7.53e-4 by using
[NH3]^2/[N2][H2]^3
but it says my answer is wrong
Just examining it, your answer is wrong.
look at the denominator; 1.6E-2*(4E-2)^2 = 25.6E-6
that E-6 turns to E6 in the numerator, which fill force the power in the numerator to be high, nowhere near e-4
recalculate.
Thanks for showing what you did. I suspect you just punched in the wrong numbers because I don't get anything close to that.
If you estimate it as
(0.3)^2/(0.02)(0.05)^3
It is about 4E5.
To calculate the value of the equilibrium constant Kp for a given reaction, you need to use the partial pressures of the reactants and products at equilibrium. The balanced equation for the reaction is:
N2(g) + 3 H2(g) ⇌ 2 NH3(g)
Using the given partial pressures:
Partial pressure of NH3 (P[NH3]) = 3.2 × 10^(-1) atm
Partial pressure of N2 (P[N2]) = 1.6 × 10^(-2) atm
Partial pressure of H2 (P[H2]) = 4.9 × 10^(-2) atm
The Kp expression for this reaction is:
Kp = [NH3]^2 / [N2][H2]^3
Substituting the given values:
Kp = (3.2 × 10^(-1))^2 / (1.6 × 10^(-2))(4.9 × 10^(-2))^3
Calculating this expression gives Kp = 7.532 × 10^(-4). So, your calculated value is correct.
If you received a different answer, there might be an error in your calculations. Please recheck your math and make sure all values and units are entered correctly.