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: Nitric acid is produced commercially by the Ostwald process. In the first step ammonia is oxidized to nitric oxide:4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g)Assume this reaction is carried out in the apparatus diagramed below.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.

Solution: Nitric acid is produced commercially by the Ostwald process. In the first step ammonia is oxidized to nitric oxide:4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g)Assume this reaction is carried out in the apparat

Problem

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

4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g)

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

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.

Solution

We are given the initial partial pressures and volumes of the reactants, we have to use the ideal gas law to calculate the moles of each. The ideal gas law can be manipulated to isolate the moles :

Now before we calculate, make sure that the units are the same as the units of the gas constant R. If not, we convert. Assume room temperature.


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