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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?Group of answer choices12.2 g10.6 g61.3 g2.13 g25.5 g

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?Group of answer choices12.2 g10.6 g61.3 g2.13 g25.5 g

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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:

  1. First, we need to find the molar mass of H2O and N2O4. The molar mass of H2O is approximately 18.015 g/mol and the molar mass of N2O4 is approximately 92.011 g/mol.

  2. Next, we need to convert the given mass of H2O (5.00 g) into moles using its molar mass.

    Moles of H2O = 5.00 g / 18.015 g/mol = 0.277 moles

  3. Now, we need to use the stoichiometric ratio from the balanced chemical equation to find the moles of N2O4 needed to produce this amount of H2O.

    From the balanced equation, we can see that 5 moles of N2O4 produce 12 moles of H2O. So, the ratio of N2O4 to H2O is 5/12.

    Moles of N2O4 = 0.277 moles H2O * (5 moles N2O4 / 12 moles H2O) = 0.115 moles N2O4

  4. Finally, we convert the moles of N2O4 back into grams using its molar mass.

    Mass of N2O4 = 0.115 moles * 92.011 g/mol = 10.6 g

So, the mass of N2O4 that would produce a theoretical yield of 5.00 g of H2O is approximately 10.6 g.

This problem has been solved

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