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Chemistry
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2NH3 —> N2 (g) + 3H2 (g)

If the total pressure of the gas at the end if the reaction is 759 mmHg, calculate the partial pressures in atm of nitrogen(N2) and hydrogen (H2)

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Related questions

Nitrogen and hydrogen gases react to form ammonia gas via the following reaction:
N2(g)+3H2(g)-->2NH3(g)
At a certain temperature and pressure, 1.4 L of N2 reacts with 4.2 L of H2.
If all the N2 and H2 are consumed, what volume of NH3, at the same temperature and pressure, will be produced?

In the Haber process, ammonia is synthesized from nitrogen and hydrogen:

N2(g) + 3H2(g) → 2NH3(g)

ΔG° at 298 K for this reaction is -33.3 kJ/mol. The value of ΔG at 298 K for a reaction mixture that consists of 1.0 atm N2, 3.0 atm H2, and 0.50 atm NH3 is ________.

In the Haber process, ammonia is synthesized from nitrogen and hydrogen:

N2(g) + 3H2(g) → 2NH3(g)

ΔG° at 298 K for this reaction is -33.3 kJ/mol. The value of ΔG at 298 K for a reaction mixture that consists of 1.0 atm N2, 3.0 atm H2, and 0.50 atm NH3 is ________.

-1.16 × 104
-44.9
-4.47 × 103
-2.0
-147.8

Kp = 0.050 for the reaction N2(g) + 3H2(g) <-> 2NH3(g) at acertain temperature. Suppose it was found that in an equilibriummixture of these gases the partial pressure of NH3(g) is 24.9 atmand the partial pressure of N2 is 6.68 atm. What is the partialpressure of H2(g)?

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