# Problem: 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, 1.6 L of N2 reacts with 4.8 L of H2.If all the N2 and H2 are consumed, what volume of NH3, at the same temperature and pressure, will be produced?

🤓 Based on our data, we think this question is relevant for Professor Pontius' class at PSU.

###### FREE Expert Solution

We are asked to calculate the volume of NH3, at the same temperature and pressure.

Since all are gases and the temperature and pressure conditions are the same, we can use the volumes as if it were moles for stoichiometry.

We do this because we are not given the pressure so we can't calculate moles and it is mathematically correct when ideal gas law is used. ###### Problem Details

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, 1.6 L of N2 reacts with 4.8 L of H2.

If all the N2 and H2 are consumed, what volume of NH3, at the same temperature and pressure, will be produced?