How many grams of water will be produced if 32.0 g of nitrous oxide are also produced in the reaction? useing this equation:
NH4NO3 (s)--> N2O (g) + 2H2O (g)
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To calculate the number of grams of water produced, we first need to determine the molar masses of nitrous oxide (N2O) and water (H2O).
The molar mass of nitrous oxide (N2O) can be calculated by adding the molar masses of nitrogen (N) and oxygen (O):
Molar mass of N2O = (2 × atomic mass of N) + atomic mass of O
= (2 × 14.01 g/mol) + 16.00 g/mol
= 28.02 g/mol + 16.00 g/mol
= 44.02 g/mol
The molar mass of water (H2O) can be calculated by adding the molar masses of hydrogen (H) and oxygen (O):
Molar mass of H2O = (2 × atomic mass of H) + atomic mass of O
= (2 × 1.01 g/mol) + 16.00 g/mol
= 2.02 g/mol + 16.00 g/mol
= 18.02 g/mol
According to the balanced equation, 1 mole of NH4NO3 will produce 2 moles of H2O. Therefore, the number of moles of H2O produced can be calculated as follows:
Number of moles of H2O = (g of N2O produced) × (1 mol of H2O / 44.02 g of N2O)
= (32.0 g) × (1 mol H2O / 44.02 g N2O)
= 0.7275 mol H2O
To convert the number of moles of H2O to grams, we can use the molar mass of water:
Number of grams of H2O = (Number of moles of H2O) × (Molar mass of H2O)
= (0.7275 mol) × (18.02 g/mol)
≈ 13.11 g
Therefore, approximately 13.11 grams of water will be produced when 32.0 grams of nitrous oxide are produced in the reaction.
To find the number of grams of water produced in the reaction, we need to determine the stoichiometric ratio between nitrous oxide (N2O) and water (H2O) in the given equation.
From the balanced equation:
NH4NO3 (s) → N2O (g) + 2H2O (g)
We can see that for every one mole of nitrous oxide produced, two moles of water are also produced. To find the number of moles of nitrous oxide (N2O), we divide the given mass of N2O by its molar mass.
First, let's calculate the molar mass of N2O:
Nitrogen (N) atomic mass = 14.01 g/mol
Oxygen (O) atomic mass = 16.00 g/mol
Molar mass of N2O = 2(14.01 g/mol) + 16.00 g/mol = 44.02 g/mol
Now we can calculate the number of moles of N2O:
Moles of N2O = Mass of N2O / Molar mass of N2O
Moles of N2O = 32.0 g / 44.02 g/mol ≈ 0.727 mol
Since the stoichiometric ratio states that 1 mole of N2O produces 2 moles of H2O, we can determine the moles of water produced:
Moles of H2O = 2 × Moles of N2O
Moles of H2O = 2 × 0.727 mol = 1.454 mol
Finally, we can convert moles of water to grams by multiplying by the molar mass of water, which is approximately 18.02 g/mol:
Grams of H2O = Moles of H2O × Molar mass of H2O
Grams of H2O = 1.454 mol × 18.02 g/mol ≈ 26.2 g
Therefore, approximately 26.2 grams of water will be produced when 32.0 grams of nitrous oxide are also produced in the reaction.