The space shuttle utilised the oxidation of methylhydrazine by dinitrogen tetroxide for propulsion. The balanced reaction is:5N2O4(l) + 4N2H3CH3(l) → 4CO2(g) + 12H2O(g) + 9N2(g)What mass of N2O4 would produce a theoretical yield of 5.00 g of H2O?
Question
The space shuttle utilised the oxidation of methylhydrazine by dinitrogen tetroxide for propulsion. The balanced reaction is:5N2O4(l) + 4N2H3CH3(l) → 4CO2(g) + 12H2O(g) + 9N2(g)What mass of N2O4 would produce a theoretical yield of 5.00 g of H2O?
Solution
To solve this problem, we need to use stoichiometry, which is a method in chemistry that uses the relationships between reactants and products in a chemical reaction to determine desired quantitative data.
Here are the steps:
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Convert the given mass of H2O to moles. The molar mass of H2O is approximately 18.015 g/mol.
5.00 g H2O * (1 mol H2O / 18.015 g H2O) = 0.277 moles H2O
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Use the stoichiometric ratio from the balanced chemical equation to find the moles of N2O4. The ratio of N2O4 to H2O is 5:12.
0.277 moles H2O * (5 mol N2O4 / 12 mol H2O) = 0.115 moles N2O4
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Convert the moles of N2O4 to grams. The molar mass of N2O4 is approximately 92.02 g/mol.
0.115 moles N2O4 * (92.02 g N2O4 / 1 mol N2O4) = 10.6 g N2O4
So, theoretically, 10.6 g of N2O4 would produce 5.00 g of H2O.
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