Ch.5 - GasesSee 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: Assume this reaction is carried out in the apparatus diagram below. Nitric acid is produced commercially by the Ostwald process. In the first step, ammonium is oxidized to nitric oxide: 4 NH 3(g) + 5 O 2(g) → 4 NO(g) + 6 H 2O(g) The stopcock between the two reaction containers is opened, and the reaction proceeds using proper catalysts. Calculate the partial pressure of NO after the reaction is complete. Assume 100% yield for the reaction, assume the final container volume is 3.00 L, and assume the temperature is constant. 1. 0.333 atm 2. 0.500 atm 3. 0.250 atm 4. 0.400 atm 5. 1.50 atm

Problem

Assume this reaction is carried out in the apparatus diagram below.

Nitric acid is produced commercially by the Ostwald process. In the first step, ammonium is oxidized to nitric oxide:

4 NH 3(g) + 5 O 2(g) → 4 NO(g) + 6 H 2O(g)

The stopcock between the two reaction containers is opened, and the reaction proceeds using proper catalysts. Calculate the partial pressure of NO after the reaction is complete. Assume 100% yield for the reaction, assume the final container volume is 3.00 L, and assume the temperature is constant.

1. 0.333 atm

2. 0.500 atm

3. 0.250 atm

4. 0.400 atm

5. 1.50 atm