A mixture of nitrogen gas, hydrogen gas and ammonia gas reacts by: N2(g) + 3H2(g) = 2NH3(g) If the total pressure in the reaction vessel is 50.0 atm ans the equilibrium mixture contains by volume: N2= 96.143% H2= 0.3506% NH3= 3.506% what is the equilibrium constant (Kp)?
I should point out that the total doesn't add up to 100% (almost but not quite) so you may want to check your problem vs your post.
%by volume = mole fraction or X.
Therefore, XN2 = 0.96143; XH2 = 0.003506; XNH3 = 0.03506
pN2 = XN2*Ptotal
pH2 = XH2*Ptotal
pNH3 = XNH3*Ptotal
Substitute the pressures into the Kp expression and solve for Kp. Post your work if you get stuck.
So I found the pressure of each one by foing 50.0 atm* 0.96 for N2 and got 48 atm. For PH2 I did 0.0035 * 50.0= 0.175 atm. For PNH3 0.03506* 50.0= 1.1753 atm, but I feel like I did something wrong because I don't know where to go from here
1. Since the values are given to more places that you have shown, I would recalculate and don't throw digits away. For example, pN2 you have only two places in your answer but more than that in the Ptotal and X. Same for H2 and NH3. Redo that.
2. Where do you go from here. As I posted, you substitute these values into the Kp expression and solve for Kp.
Kp = p^2NH3/pN2*p^3H2
Remember to check your post against your problem to make sure those numbers are right.
To find the equilibrium constant (Kp) for the given reaction, you can make use of the partial pressures of the gases at equilibrium.
From the given information, we can calculate the partial pressures of nitrogen (N2), hydrogen (H2), and ammonia (NH3).
- First, let's consider the partial pressure of nitrogen (N2):
The volume percent of nitrogen gas is given as 96.143%. Therefore, the partial pressure of N2 can be calculated by multiplying the given volume percent by the total pressure:
P(N2) = (96.143 / 100) * 50.0 atm
- Next, let's calculate the partial pressure of hydrogen (H2):
The volume percent of hydrogen gas is given as 0.3506%. Therefore, the partial pressure of H2 can be calculated by multiplying the given volume percent by the total pressure:
P(H2) = (0.3506 / 100) * 50.0 atm
- Finally, let's calculate the partial pressure of ammonia (NH3):
The volume percent of ammonia gas is given as 3.506%. Therefore, the partial pressure of NH3 can be calculated by multiplying the given volume percent by the total pressure:
P(NH3) = (3.506 / 100) * 50.0 atm
Now that you have the partial pressures of N2, H2, and NH3, you can write the expression for the equilibrium constant (Kp). In this case, the equilibrium constant expression is:
Kp = (P(NH3))^2 / (P(N2) * P(H2)^3)
Substitute the calculated partial pressures into the expression, and solve for Kp.