A fuel mixture used in the early days of rocketry contained hydrazine (N2H4) and dinitrogen tetraoxide (N2O4). When ignited, the mixture released energy and produced elemental nitrogen and water: 2 N2H4(l)  +  N2O4(g)   →   3 N2(g)   +    4 H2O(g)       [balanced] What is the percent yield when 9.15 mol N2H4 reacts with 3.12 mol of N2O4 to form 7.68 mol of N2?

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Q: A fuel mixture used in the early days of rocketry contained hydrazine (N2H4) and dinitrogen…

A: Given;

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Q: Sucrose (C₁₂H₂₂O₁₁) is combusted in air according to the following reaction: C₁₂H₂₂O₁₁(s) + O₂(g) →…

A: Given :  Mass of sucrose = 35.4 gram  Molar mass of sucrose = 342 gm/mole

Q: How many moles of O₂ would be required to generate 13.0 mol of NO₂ in the reaction below assuming…

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Q: A sample of 1.544moles of methane (CH4) is mixed with 1.273 moles of chlorine. What is the…

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Q: In the following reaction, identify the limiting reactant: C3H8 (g) + 5 O2 (g) → CO2 (g) + 2 H2O…

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A: Percent yield = actual yield / theoretical yield x 100%.

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Q: What is the mass in grams of H₂ that can be formed from 31.6 grams of NH₃ in the following reaction?…

A: The number of moles, nNH3, of NH3 equivalent to 31.6 g of NH3 is; nNH3=mNH3MMNH3=31.6 g17.03…

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A: Mass of NH3 = 34.0 g Mass of H2 = ?

Q: Determine the theoretical yield of HCl

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Q: what is the percent yield?

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Q: Calculate the percent yield if 10.8 g of nitrogen gas is produced from the decomposition of 41.9 g…

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Q: consider the following balanced equation. N2O4(l) + 2 N2H4(l)  →  3 N2(g) + 4 H2O(g) Determine the…

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Q: What is the mass in grams of H₂ that can be formed from 43.6 grams of NH₃ in the following reaction?…

A: Molar mass of NH3 = Atomic mass of N + H x 3                                = 14 g/mol + 1 g/mol x 3…

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Q: A reaction of 58.3 g of Na and 56.5 g of Br, yields 58.3 g of NaBr. What is the percent yield? 2…

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