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

3H2+N2-2NH3
How many grams of are needed to produce 13.75g of NH3 ?
How many molecules (not moles) of are produced from 8.26×10−4g of H2 ?

Your question is better but it still needs work. Howmany grams of ???? are needed to produce etc.

4.14 x 10^19

H2 is the limiting reagent

grams of NH3 is 102g

To answer these questions, we need to use stoichiometry, which relates the amounts of reactants and products in a balanced chemical equation.

For the first question, we want to determine how many grams of nitrogen gas (N2) are needed to produce 13.75g of ammonia gas (NH3).

Step 1: Start by writing out the balanced chemical equation:
3H2 + N2 → 2NH3

Step 2: Calculate the molar mass of ammonia:
NH3 = 14.01 g/mol (1 nitrogen atom) + 3(1.01 g/mol) (3 hydrogen atoms)
NH3 = 17.04 g/mol

Step 3: Use the molar ratios from the balanced equation to find the amount of nitrogen needed:
From the balanced equation, we know that 3 moles of hydrogen gas reacts with 1 mole of nitrogen gas to produce 2 moles of ammonia gas. Therefore, the molar ratio of N2 to NH3 is 1:2.

Step 4: Convert the grams of ammonia to moles:
13.75 g NH3 * (1 mol NH3 / 17.04 g NH3) = 0.806 mol NH3

Step 5: Use the molar ratio to find the moles of nitrogen:
Since the ratio of N2 to NH3 is 1:2, for every 2 moles of NH3, we need 1 mole of N2.
0.806 mol NH3 * (1 mol N2 / 2 mol NH3) = 0.403 mol N2

Step 6: Convert moles of nitrogen to grams:
0.403 mol N2 * (28.02 g N2 / 1 mol N2) = 11.29 g N2

Therefore, 11.29 grams of N2 are needed to produce 13.75 grams of NH3.

For the second question, we want to determine the number of molecules of ammonia (NH3) produced from 8.26×10−4g of hydrogen gas (H2).

Step 1: Start by writing out the balanced chemical equation (already given):
3H2 + N2 → 2NH3

Step 2: Calculate the molar mass of hydrogen gas:
H2 = 2(1.01 g/mol) = 2.02 g/mol

Step 3: Convert the grams of hydrogen gas to moles:
8.26×10−4 g H2 * (1 mol H2 / 2.02 g H2) = 4.08×10−4 mol H2

Step 4: Use the molar ratio from the balanced equation to find the moles of NH3:
According to the balanced equation, 3 moles of H2 react to produce 2 moles of NH3. Therefore, the molar ratio of H2 to NH3 is 3:2.
4.08×10−4 mol H2 * (2 mol NH3 / 3 mol H2) = 2.72×10−4 mol NH3

Step 5: Convert moles of NH3 to molecules:
1 mol NH3 contains Avogadro's number (6.022×10^23) molecules of NH3.
2.72×10−4 mol NH3 * (6.022×10^23 molecules NH3 / 1 mol NH3) = 1.64×10^20 molecules NH3

Therefore, 1.64×10^20 molecules of NH3 are produced from 8.26×10−4g of H2.