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1) Hydrazine, N2H4, once used as a rocket propellant, reacts with oxygen in the following equation. -> N2H4(g) + O2(g) → N2(g) + 2 H2O(g) The reaction, at 50% yield, produces 4.0 moles of N2. What was the mass of hydrazine used? Assume that O2 is in excess. A) 64 g cal for B) 32.0 g C) 260 g D) 0.063 g

1) Hydrazine, N2H4, once used as a rocket propellant, reacts with oxygen in the following equation. -> N2H4(g) + O2(g) → N2(g) + 2 H2O(g) The reaction, at 50% yield, produces 4.0 moles of N2. What was the mass of hydrazine used? Assume that O2 is in excess. A) 64 g cal for B) 32.0 g C) 260 g D) 0.063 g

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter3: Equation, The Mole, And Chemical Formulas
Section: Chapter Questions
Problem 3.129QE
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1) Hydrazine, N2H4, once used as a rocket propellant, reacts with oxygen in the following equation. -> N2H4(g) + O2(g) → N2(g) + 2 H2O(g) The reaction, at 50% yield, produces 4.0 moles of N2. What was the mass of hydrazine used? Assume that O2 is in excess. A) 64 g cal for B) 32.0 g C) 260 g D) 0.063 g
Transcribed Image Text:1) Hydrazine, N2H4, once used as a rocket propellant, reacts with oxygen in the following equation. -> N2H4(g) + O2(g) → N2(g) + 2 H2O(g) The reaction, at 50% yield, produces 4.0 moles of N2. What was the mass of hydrazine used? Assume that O2 is in excess. A) 64 g cal for B) 32.0 g C) 260 g D) 0.063 g
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