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A fuel mixture used in the early days of rocketry consisted of hydrazine (N,H4) and dinitrogen tetroxide (N204), which ignite on contact to form nitrogen gas and water vapour: 2 N2H4() + N204(h→ 3 N2(8) + 4 H20(e) Molar mass of N,H4= 32.05 g/mol Molar mass of N204=92.02 g/mol Molar mass of N,= 28.02 g/mol Molar mass of H2O= 18.02 g/mol a. What mass (in grams) of nitrogen gas is form when 1.00 x 10 g of N,H4 and 2.00 x 10 g of N,O4 are mixed? AND specify what is the limiting reactant. Limiting reactant = FINAL ANSWER: b. What mass (in grams) of the excess reactant remains after the reaction is complete? FINAL ANSWER: 1. The limiting reactant is (give the chemical formula) = A 2. Mass of N2 produced (include units): A 3. Excess reactant left over (include units) =

A fuel mixture used in the early days of rocketry consisted of hydrazine (N,H4) and dinitrogen tetroxide (N204), which ignite on contact to form nitrogen gas and water vapour: 2 N2H4() + N204(h→ 3 N2(8) + 4 H20(e) Molar mass of N,H4= 32.05 g/mol Molar mass of N204=92.02 g/mol Molar mass of N,= 28.02 g/mol Molar mass of H2O= 18.02 g/mol a. What mass (in grams) of nitrogen gas is form when 1.00 x 10 g of N,H4 and 2.00 x 10 g of N,O4 are mixed? AND specify what is the limiting reactant. Limiting reactant = FINAL ANSWER: b. What mass (in grams) of the excess reactant remains after the reaction is complete? FINAL ANSWER: 1. The limiting reactant is (give the chemical formula) = A 2. Mass of N2 produced (include units): A 3. Excess reactant left over (include units) =

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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A fuel mixture used in the early days of rocketry consisted of hydrazine (N,H4) and dinitrogen tetroxide (N204), which ignite on contact to form nitrogen gas and water vapour: 2 N2H4() + N204(1) → 3 N2(8) + 4 H2O(e) Molar mass of N,H4= 32.05 g/mol Molar mass of N,04=92.02 g/mol Molar mass of N,= 28.02 g/mol Molar mass of H2O= 18.02 g/mol a. What mass (in grams) of nitrogen gas is form when 1.00 x 10 g of N,H4 and 2.00 x 10 g of N,04 are mixed? AND specify what is the limiting reactant. Limiting reactant = FINAL ANSWER: b. What mass (in grams) of the excess reactant remains after the reaction is complete? FINAL ANSWER: 1. The limiting reactant is (give the chemical formula) = A 2. Mass of N2 produced (include units): A 3. Excess reactant left over (include units) = What is the mass percent (percent composition) of hydrogen (H) in glucose (C6H1206)? Give the answer with 2 significant figures. FINAL ANSWER:
Transcribed Image Text:A fuel mixture used in the early days of rocketry consisted of hydrazine (N,H4) and dinitrogen tetroxide (N204), which ignite on contact to form nitrogen gas and water vapour: 2 N2H4() + N204(1) → 3 N2(8) + 4 H2O(e) Molar mass of N,H4= 32.05 g/mol Molar mass of N,04=92.02 g/mol Molar mass of N,= 28.02 g/mol Molar mass of H2O= 18.02 g/mol a. What mass (in grams) of nitrogen gas is form when 1.00 x 10 g of N,H4 and 2.00 x 10 g of N,04 are mixed? AND specify what is the limiting reactant. Limiting reactant = FINAL ANSWER: b. What mass (in grams) of the excess reactant remains after the reaction is complete? FINAL ANSWER: 1. The limiting reactant is (give the chemical formula) = A 2. Mass of N2 produced (include units): A 3. Excess reactant left over (include units) = What is the mass percent (percent composition) of hydrogen (H) in glucose (C6H1206)? Give the answer with 2 significant figures. FINAL ANSWER:
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