Question

in a 3 L vessel, the following equilibrium pressure are measured, N2 = 100 mm of Hg, H2= 400 mm of Hg, and NH3= 1000 mm of Hg . nitrogen is removed from the vessel at constant temperature until the pressure of hydrogen at equilibrium pressure is equal to 700 mm oh Hg, the new equilibrium partial pressure of N2 is​

Answer 1

The new equilibrium partial pressure of N2 is​ 200 torr.

Explanation:

The reaction between nitrogen gas and hydrogen gas is given below.

N2(g) + 3H2 (g) ---> 2 NH3 (g)

At the equilibrium, the partial pressure of nitrogen gas is 100 torr, hydrogen gas is 400 torr and ammonia gas is 1000 torr.

Partial pressure of nitrogen gas can be calculated as:

100 torr + 3P = 700 torr

3P = 700 torr - 100 torr

3P = 600 torr

P = 600 / 3 = 200 torr

Thus the new equilibrium partial pressure of N2 is​ 200 torr.

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