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Nitrogen and hydrogen gases react to form ammonia gas as follows:

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

At a certain temperature and pressure, 1.2 L of N2 reacts with 3.6 L of H2. If all the N2 and H2 are consumed, what volume of NH3, at the same temperature and pressure, will be produced?

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Jamar Ferry
Jamar FerryLv2
23 May 2020

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Related questions

Ammonia gas is synthesized according to the balanced equation below. N2(g) + 3 H2(g) -> 2 NH3(g) If 2.50 L N2 react with 7.00 L H2, what is the theoretical yield (in liters) of NH3? Assume that the volumes of reactants and products are measured at the same temperature and pressure.

Reaction of hydrogen and nitrogen to form ammonia
Hydrogen gas, H2, reacts with nitrogen gas, N2, to form ammonia gas, NH3, according to the equation

3H2(g)+N2(g)→2NH3(g)

NOTE: Throughout this tutorial use molar masses expressed to five significant figures.

1. How many grams of NH3 can be produced from 2.66 mol of N2 and excess H2.

2. How many grams of H2 are needed to produce 13.24 g of NH3?

3.How many molecules(not moles) of NH3 are produced from 1.43×10−4 g of H2?

Hydrogen gas, H2, reacts with nitrogen gas, N2, to form ammonia gas, NH3, according to the equation

3H2(g)+N2(g)→2NH3(g)

1)How many grams of H2 are needed to produce 10.85 g of NH3?

2)How many molecules (not moles) of NH3 are produced from 3.23×10−4 g of H2?

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