# Equilibrium Pressure

## Homework Statement

H2 (g) + Cl2(g) $$\Updownarrow$$ 2HCl (g) Kp = 2.5 × 1033
NH3(g) + HCl(g) $$\Updownarrow$$ NH4Cl(s) Kp = 2.1 × 1015
N2(g) + 4H2(g) +Cl2 $$\Updownarrow$$ 2NH4Cl(s) Kp = 3.9 × 1070

Determine the Kp for N2(g) + 3H2 (g) $$\Updownarrow$$ 2NH3(g).

Don't know/none

## The Attempt at a Solution

In order to get to N2(g) + 3H2 (g) $$\Updownarrow$$ 2NH3(g), I would have to multiple/flip equations so that they result in the desired reaction set.
-(H2 (g) + Cl2(g) $$\Updownarrow$$ 2HCl (g) Kp = 2.5 × 1033)
-2(NH3(g) + HCl(g) $$\Updownarrow$$ NH4Cl(s) Kp = 2.1 × 1015)
N2(g) + 4H2(g) +Cl2 $$\Updownarrow$$ 2NH4Cl(s) Kp = 3.9 × 1070

These would cancel out to the desired reaction.

In Hess's Law, I understand that multiplying a step would mean its enthalpy gets multiplied by that number. If I flip a step, its enthalpy would inverse its sign.

In voltage calculation from standard reduction potentials, reversing the sign would inverse the potential for the step but multiplying the step does not affect the potential.

Originally I would just follow Hess's Law to calculate but I never did this for Kp and so I'm not sure the answer would be correct. How do I approach this problem and solving for Kp.