(a)
Interpretation-To determine the partial pressure of
Introduction- Ideal
Where, P = pressure in
R = universal gas constant =
Limiting Reactant -It is the reactants that finish first when the reaction stops and limits the amount of product formation.
(a)
Answer to Problem 94A
The partial pressure of
Explanation of Solution
Given:
Mass of
Mass of
Molar mass of
Molar mass of
Mole ratio of
Mole ratio of
- Limiting reactant can be found as:
- Partial pressure can be calculated using the ideal gas law as:
a. Amount of
b. Amount of produced by can be calculated as:
Hence, the limiting reactant is ammonia as it produced a lesser amount of product.
The theoretical yield of
Given:
Volume =
Temperature =
Mole =
Therefore, the partial pressure of
Therefore, the partial pressure of
(b)
Interpretation- To determine the total pressure
Introduction-
When the reactant stops, product and excess reactants remain.
Excess reactant is the reactant that remains when the reaction stops. The amount of excess reactant can be calculated using stoichiometry.
The total pressure can be calculated using Dalton’s Law of partial pressure:
Where P total =total pressure
P1,P2,P3 are partial pressure of gases.
(b)
Answer to Problem 94A
Therefore, the total pressure in the container = 4.43atm
Explanation of Solution
Oxygen gas is an excess reactant as ammonia is calculated as limiting. So, oxygen gas, nitrogen monoxide, and water remain when the reaction stops.
Amount of oxygen gas reacted:
Partial pressure of oxygen gas can be calculated as:
Amount of water produced:
Partial pressure of water
Total pressure can be calculated as:
Chapter 14 Solutions
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