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I think it's due to an error in calculation somewhere.
To solve this question, you'll have to use the information provided,
"N2(g) + 3H2(g) ⇌ 2NH3(g)When equilibrium was reached, the total pressure in the flask was 150 kPa and themole fraction of NH3(g) in the mixture was 0.80."Firstly, calculate the partial pressure of ammonia by using the formula,
partial pressure of ammonia = mole fraction of ammonia x total pressure in the flaskAnswer: partial pressure of ammonia is 120kPa.
Hence, we know that the partial pressure of the nitrogen and hydrogen added up would be 150kPa-120kPa, 30kPa in total.
Secondly, calculate the individual mole fractions of hydrogen and nitrogen.
Since ammonia's mole fraction is 0.8, it means, 0.8/1 moles of gas in the flask is ammonia.
Hence, from this, we know that the remaining 0.2 moles of gas are nitrogen/ hydrogen.
Using the information above...
Since we know that nitrogen and hydrogen combine in a 1:3 ratio, the mole fraction of nitrogen would be (3/4) the remaining moles of gas,
(3/4)x0.2 and, the mole fraction of hydrogen would be (1/4) the remaining moles of gas, (1/4)x0.2
Then, use the formula, partial pressure of gas A = mole fraction of gas A x total pressure in the system to solve for the partial pressure of nitrogen and hydrogen.