# Frequent question: How many moles of ammonia are produced?

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## How do you find the number of moles produced?

Determine the moles of product produced by dividing the grams of product by the grams per mole of product. You now have calculated the number of moles of every compound used in this reaction.

## How many moles of NH3 gas are produced?

Using the proportions of the amount of the molecules, we can convert from any reagent or product to any other reagent or product. In the context of this reaction, for every mole of N2 and every 3 moles of H2 we obtain 2 moles of NH3.

## How many moles of ammonia can be produced from 8moles of nitrogen gas?

Therefore 9 moles of nitrogen are required to produce 18 moles of ammonia.

## How do you calculate product production?

Find the limiting reagent by calculating and comparing the amount of product each reactant will produce.

1. Balance the chemical equation for the chemical reaction.
2. Convert the given information into moles.
3. Use stoichiometry for each individual reactant to find the mass of product produced.
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## How many moles of water are produced when 5 moles of oxygen are consumed?

Then, there are 2 moles of water produced every time that 5 moles of oxygen react with 2 moles of acetylene.

## How many grams of ammonia are produced from 3.0 moles of nitrogen?

Nam D. Nitrogen is the limiting reactant, and 3.74 grams of ammonia is formed.

## How many moles of NH3 are produced when 13 moles of H2 react?

How many moles of NH3 are produced when 1.3 mol of H2 reacts? According to the reaction equation from 3 mol of H2 be produced 2 moles of NH3. Answer: 0.87 moles of NH3 are produced from 1.3 moles of H2.

## How many moles of NH3 are produced when 2.1 moles H2 reacts?

How many moles of NH3 are produced when 2.1 mol of H2 reacts? Solution. x = 2,1*2/3 = 1,4 mol.

## How many moles of Cl2 are produced from 4 moles HCl?

It is 4 moles HCl to 1 mole O2. Calculate moles of each and see which is limiting. To obtain theoretical yield, you use the reactant that is limiting and the mole ratio of that reactant to the product. For example, if HCl is limiting, then 4 moles HCl produces 2 moles Cl2.