Question

a. calculate the mass of dinitrogen tetroxide required to completely react with 100.0g of hydrazine.

b. calculate the masses of the two products that would result from the reaction of 100.0g of hydrazine.

Answer 1

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dinitrogen tetraoxide (NO) and hydrazine (NH4). The reaction blo both the reactants 12N, HAT N₂O4 ( 3N₂ + 4H2O(1) NH4 & Mass 100.0g ; molar Mass = 32.04 g/mol mass molar mass no. of moles = 100.09 32.04 g/mol = 3.12 mof From equation & a mol N₂H₂ reacts with 1 mol NOA (2:1 mol ratio) so 3.12 mol Nat4 reacts with mol N04 - 3.12 mol x I mot - = 1.56 md of N.04. 2 mol # Mass of N = no. of moles & molar mass = 1.56 mol X 92.01 g/mol = 143.589 of 1,04 is required 6 Here products are Nitrogen gas and water 2 mol Not reacts to produce 3 mol N (2:3 ratio) go, 3.12 mol Natte reacts to produce – mol No . → 3.12 mol x 3 mol = 4.68 mol 2 mol mass of N = nx mom of N = 4.68 mol x 28.01g/mol -]131.08916 Ny will be produced ant, a mot Notty reacts to produce 4 mol of H20 (2:45182 mol ratio 30 3-12 ml Nth reacts to produce – mot of the > 3. 12 mol x 4 mol = 6.24 mot 2 moi Mass of H₂O = 6.24 mol x 18.01 g/mol [112.38 g of He will be produced