A mixture of 3.00 volumes of H2 and 1.00 volume of N2 reacts at 344 C to form ammonia. The equilibrium mixture at 110.0 atm contains 47.00 % NH3 by volume. Calculate Kp for the reaction, assuming that the gases behave ideally.

I'm not understanding what you mean "ratios in the end" but if you want to post your work/answers I can check it. I went through mole fractions and calculated partial pressure of each gas, substituted that into the Kp expression and solve for Kp.

Oh.. I figured it out. So you should do stoichiometry in ratios, very accurately, by solving for the one unknown in the end. Then just multiply found ratios by 110 and find Kp from the equilibrium pressures.

To calculate Kp for the reaction, we need to use the equation:

Kp = (P(NH3))^2 / (P(H2))^3 * (P(N2))

Given:
Volume of H2 = 3.00 volumes
Volume of N2 = 1.00 volume
Equilibrium mixture volume = 47.00 % NH3 by volume
Equilibrium pressure = 110.0 atm

Step 1: Convert percentages into volumes

Since the equilibrium mixture is given in terms of volume percentage, we need to convert it into volumes. Assuming the total volume of the mixture is 1.00 volume, the volume of NH3 would be 0.4700 volumes.

Step 2: Calculate the partial pressures

We can calculate the partial pressures of each gas using the ideal gas law:

PV = nRT

For NH3:
P(NH3) = (0.4700 * 110.0) / 1.00 = 51.70 atm

For H2:
P(H2) = (3.00 * 110.0) / 1.00 = 330.0 atm

For N2:
P(N2) = (1.00 * 110.0) / 1.00 = 110.0 atm

Step 3: Calculate Kp

Using the equation for Kp:

Kp = (P(NH3))^2 / (P(H2))^3 * (P(N2))
= (51.70^2) / (330.0^3 * 110.0)

This gives us the value of Kp for the reaction.

To calculate Kp for the reaction, we need to first write the balanced equation.

The balanced equation for the reaction is:
N2(g) + 3H2(g) ⇌ 2NH3(g)

From the given information, we know the initial volumes of the reactants and the composition of the equilibrium mixture in terms of NH3.

1. Calculate the initial moles of each gas:
Since the volumes of gases are given, we can use the ideal gas law to convert the volumes to moles.

For H2:
Using the ideal gas law: PV = nRT
n(H2) = (P(H2) * V(H2)) / (R * T)
where P(H2) is the pressure of H2, V(H2) is the volume of H2, R is the ideal gas constant, and T is the temperature.

Substituting the values:
n(H2) = (110.0 atm * 3.00 L) / (0.0821 atm L/mol K * 344 K)

Similarly, calculate the moles of N2:
n(N2) = (110.0 atm * 1.00 L) / (0.0821 atm L/mol K * 344 K)

2. Calculate the equilibrium moles of NH3:
The composition of the equilibrium mixture is given as 47.00% NH3 by volume. We can assume the total volume of the mixture to be 1 L.

Since NH3 is a product with a coefficient of 2 in the balanced equation, its volume will be 47.00% * 1 L * 2 = 0.94 L

3. Calculate Kp:
Kp can be calculated using the formula:
Kp = (P(NH3))^2 / (P(N2) * P(H2)^3)
where P(NH3), P(N2), and P(H2) are the partial pressures of NH3, N2, and H2, respectively.

Since the gases behave ideally, we can assume their partial pressures are proportional to their moles.

Substituting the values, we get:
Kp = (n(NH3) / V(total))^2 / (n(N2) / V(total) * (n(H2) / V(total))^3)

Now, substitute the calculated values of moles and volume into the equation to get the value of Kp.

Note: Please ensure that you have used the correct values with the appropriate units and gas constant.