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**1. Homework Statement**

A 1L flask is filled with 1 mole of H2 and 2 moles of I2 at 448degrees Celcius. The value of the Keq for the reaction

H2 + I2 -><- 2HI at 448degrees Celcius is 50.5. What are the partial pressures of H2, I2, and HI in the flask at Equilibrium?

All reactants and products are gases. Answer is to be in atm.

**2. Homework Equations**

PV=nRT

Pressure of:

H2 I2 HI

I

C

E

**3. The Attempt at a Solution**

First, the initial equilibrium of HI is 0 because it doesnt exist yet.

I used PV=nRT to find pressure of H2 and I2

H2) P= 1mole x .0821 x 721K

------------------------- = 59.19atm

1L

I2) P= 2mole x .0821 x 721K

---------------------- = 118.39atm

1L

I need help trying to find what exactly happens after the system reaches equilibrium and how to find the final pressures. Thought: could the pressure of H2 be the same before and after equilibrium because the temperature remains the same? Same for I2?