170 kg = 170,000g NH3 = 170,000g / 17.0g/molNH3 = [10,000 molNH3] * 3moleH2 / 2moleNH3
= 15,000 mole H2 needed to produce 170 kg NH3
The reaction of nitrogen with hydrogen to form ammonia is: N2 +3H2 = 2NH3 Therefore to make 10 moles of ammonia you need 5 moles N2 and 15 moles H2
N2 + 3H2 -----> 2NH3 so 3 moles of hydrogen produce 2 moles of ammonia. Therefore 12.0 moles of hydrogen will produce 8 moles of ammonia.
3H2 + N2 <------> 2NH3 is the balanced equation for Hydrogen and Nitrogen making ammonia. 3 moles of H2 produces two moles of ammonia and thus to make 6 moles requires 9 moles of Hydrogen.
2N + 3H2 -> 2NH3 18 moles H2 (2 moles NH3/3 moles H2) = 12 mole ammonia
N2 + 3H2 -> 2NH3 The stoichiometric equation (or balanced equation) for the formation of ammonia from this we can read off the mole ratio between hydrogen and ammonia; 3M H2 needed to produce 2M NH3 times each by 9 (so the ratio remains the same and 18M NH3 is formed) 27M H2 needed to produce 18M NH3
The reaction of nitrogen with hydrogen to form ammonia is: N2 +3H2 = 2NH3 Therefore to make 10 moles of ammonia you need 5 moles N2 and 15 moles H2
N2 + 3H2 -----> 2NH3 so 3 moles of hydrogen produce 2 moles of ammonia. Therefore 12.0 moles of hydrogen will produce 8 moles of ammonia.
That amount of ammonia contains two moles of hydrogen gas. One mole of hydrogen gas weighs 2.016 grams. Therfore 3.75 grams of ammonia contains two moles of hydrogen.
N2 + 3H2 -> 2NH3 3 moles hydrogen gas. You should know that because of the formula of ammonia.
This is based on calculations too. It contains 18 hydrogen moles.
3H2 + N2 <------> 2NH3 is the balanced equation for Hydrogen and Nitrogen making ammonia. 3 moles of H2 produces two moles of ammonia and thus to make 6 moles requires 9 moles of Hydrogen.
2N + 3H2 -> 2NH3 18 moles H2 (2 moles NH3/3 moles H2) = 12 mole ammonia
N2 + 3H2 -> 2NH3 The stoichiometric equation (or balanced equation) for the formation of ammonia from this we can read off the mole ratio between hydrogen and ammonia; 3M H2 needed to produce 2M NH3 times each by 9 (so the ratio remains the same and 18M NH3 is formed) 27M H2 needed to produce 18M NH3
To form ammonia, balanced reaction is N(2) + 3H(2) ---> 2NH(3) + H(2)O. As you can see for 1 mole of nitrogen three moles of hydrogen is required. Hence for your question, 3 moles nitrogen is required to satisfy the ratio.
According balanced equation ,3 mols are needed. So 3mol shoul be mixed
4NH3 + 3O2 -----> 2N2 + 6H2O 4 moles of ammonia react with 3 of oxygen. So 10 moles of ammonia requires 7.5 moles of oxygen.
First you have to find the limiting reactant. You have .3 moles of nitrogen and .6 moles of hydrogen, but you don't know which one is going to run out first.In any of these stoichiometry problems, you need to write down the formula:N2 + 3H2 → 2NH3Take both nitrogen and hydrogen and figure out how much ammonia is made alone..6 moles Hydrogen ÷ 3 moles hydrogen × 2 moles ammonia = .4 moles ammonia made.3 moles Nitrogen ÷ 1 mole nitrogen × 2 mole ammonia = .6 moles ammonia madeNow you figured out that hydrogen is the limiting reactant and the nitrogen is the excess because less ammonia is made using hydrogen. This measurement is what you will be using for the rest of the problem.Take the limiting reactant and use stoichiometry to find how much ammonia can be made.You could start with .6 moles of hydrogen and do the same conversion as above, but add the step of converting to grams. Or, since you already found out that .4 moles ammonia is made, just convert it to grams. The molecular mass of ammonia is 17.0 grams..4 moles ammonia × 17.0 grams = 6.8 grams ammonia