(a)
Interpretation:
Rate law for the reaction of nitrogen monoxide with hydrogen has to be given.
(a)
Answer to Problem 13.99QE
Rate law for the given reaction is
Explanation of Solution
The reaction between nitrogen monoxide and hydrogen to produce nitrogen and water is given be the equation shown below;
Relative concentration of the reactant is determined by dividing the pressure of each reactant by the smallest pressure of the reactant. Relative rate of the reaction is determined by dividing the rate of the reaction by the smallest rate that is obtained from the experimental data.
The relative concentration in terms of pressure of
Initial | Initial | Initial rate of the reaction | Relative | Relative | Relative rates of the reaction |
From the above table, it is found that in experiments 1, 2 and 3, the concentration of nitrogen monoxide remains constant while the relative rate of the reaction increases in relative manner as the concentration of
From the above table, it is found that in experiments 4, 5 and 6, the concentration of hydrogen remains constant while the relative rate of the reaction doubles as the concentration of
Rate law:
Rate law is the relationship between the concentration of the reactants and the rate of the reaction. The rate law equation is given as the rate of the reaction that is directly proportional to the product of the reactant concentration that is raised to the power of the respective reactant coefficient. Therefore, the rate law for the given reaction is as follows;
Where,
(b)
Interpretation:
Rate constant for the reaction of nitrogen monoxide with hydrogen has to be given.
(b)
Answer to Problem 13.99QE
Rate constant for the given reaction is
Explanation of Solution
The rate law for the given reaction is as follows;
Where,
Rate constant:
The rate constant for the reaction can be calculated from the rate law using the initial pressure of the reactants as shown below;
Rearranging the above equation in order to calculate the rate constant;
Substituting the values for rate and the pressure of the reactants in the above equation, the rate constant of the reaction is calculated as shown below;
Therefore, the rate constant for the reaction is
(c)
Interpretation:
Activation energy has to be calculated for the reaction of nitrogen monoxide with hydrogen.
Concept Introduction:
Activation energy is the minimum amount of energy that has to be possessed by the reactant species in order to produce products. Activation energy is represented as
(c)
Answer to Problem 13.99QE
Activation energy of the reaction is
Explanation of Solution
The relative rate constants and temperature are as follows;
Rate constant | Temperature |
Activation energy and the rate constants for a reaction at two different temperatures is related by the equation as follows;
Where,
Rearranging equation (1) in order to obtain activation energy, the equation is given as shown below;
Substituting the first and third entry from the table given above in equation (2), the activation energy can be calculated as follows;
Therefore, the activation energy of the reaction is
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Chapter 13 Solutions
Chemistry: Principles and Practice
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