Ch.3 - Chemical ReactionsWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: Hydrazine, N2H4, is an oily liquid used as a rocket fuel. It can be prepared in water by oxidizing ammonia with hypochlorite ions:2 NH3(g) + ClO(aq) → N2H4(aq) + Cl(aq) + H2O(l)When 35.0 g of ammonia reacted with excess hypochlorite ion, 25.2 g of hydrazine was produced. What is the percent yield of hydrazine?(A) 76.5% (B) 68.3% (C) 17.1% (D) 19.1% (E) 72.0%

Problem

Hydrazine, N2H4, is an oily liquid used as a rocket fuel. It can be prepared in water by oxidizing ammonia with hypochlorite ions:

2 NH3(g) + ClO(aq) → N2H4(aq) + Cl(aq) + H2O(l)

When 35.0 g of ammonia reacted with excess hypochlorite ion, 25.2 g of hydrazine was produced. What is the percent yield of hydrazine?

(A) 76.5% 

(B) 68.3% 

(C) 17.1% 

(D) 19.1% 

(E) 72.0%

Solution

Use stoichiometry to determine the actual yield from 35 g NH3 and eventually the percent yield for hydrazine

Recall that percent yield is given by:

Solution BlurView Complete Written Solution