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

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter3: Stoichiometry

Section: Chapter Questions

Problem 127E: Hydrogen cyanide is produced industrially from the reaction of gaseous ammonia, oxygen, and methane:...

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