Which statements are true in the following choice? Select all that apply Questio
ID: 877805 • Letter: W
Question
Which statements are true in the following choice? Select all that apply
Question 4 options:
Determination of the orders and the rate constant of the reaction makes it possible to determine the rate law of the reaction which r = 5000 / [NO] * [H2]^2. The fact the rates of the reaction is correlated to the initial concentrations indicates that the experiment studies the integrated rate law for the reaction between NO and H2.
In the expression of the rate law, as the reaction progresses the amounts of NO and H2
Decrease which means that they are the variables of the law, while the rate constant and the reaction orders do not change throughout the reaction, which means that they are the constants of the rate law.
Determination of the orders and the rate constant of the reaction makes it possible to determine the rate law of the reaction which r = 5000 [NO]^2 * [H2]. The fact the rates of the reaction is correlated to the initial concentrations indicates that the experiment studies the differential rate law for the reaction between NO and H2.
In the expression of the rate law, as the reaction progresses the amounts of NO and H2
Decrease which means that they are the variables of the law, while the rate constant and the reaction orders do not change throughout the reaction, which means that they are the constants of the rate law.
Refer to the table and the graphs for reaction 3 for the following questions.
Using the straight line plot makes it possible to determine a parameter which is not given in the data. That parameter is the energy of activation, which is found using the following expression: R x (ln(k2) - ln(k1))/ (1/T1 -1/T2)
Refer to the table and the graphs for reaction 3 for the following questions.
Using the straight line plot makes it possible to determine a parameter which is not given in the data. That parameter is the energy of deactivation, which is found using the following expression: R / (ln(k2) - ln(k1)) x (1/T1 -1/T2)
Examination of the correct answer to the previous question shows that the equality between the rate constants would bring the value of Ea to 0, which corresponds to the most difficult, and therefore the slowest reaction.
Examination of the correct answer to the previous question shows that the equality between the rate constants would bring the value of Ea to 0, which corresponds to the easiest, and therefore the fastest reaction.
Determination of the orders and the rate constant of the reaction makes it possible to determine the rate law of the reaction which r = 5000 / [NO] * [H2]^2. The fact the rates of the reaction is correlated to the initial concentrations indicates that the experiment studies the integrated rate law for the reaction between NO and H2.
In the expression of the rate law, as the reaction progresses the amounts of NO and H2
Decrease which means that they are the variables of the law, while the rate constant and the reaction orders do not change throughout the reaction, which means that they are the constants of the rate law.
Determination of the orders and the rate constant of the reaction makes it possible to determine the rate law of the reaction which r = 5000 [NO]^2 * [H2]. The fact the rates of the reaction is correlated to the initial concentrations indicates that the experiment studies the differential rate law for the reaction between NO and H2.
In the expression of the rate law, as the reaction progresses the amounts of NO and H2
Decrease which means that they are the variables of the law, while the rate constant and the reaction orders do not change throughout the reaction, which means that they are the constants of the rate law.
Refer to the table and the graphs for reaction 3 for the following questions.
Using the straight line plot makes it possible to determine a parameter which is not given in the data. That parameter is the energy of activation, which is found using the following expression: R x (ln(k2) - ln(k1))/ (1/T1 -1/T2)
Refer to the table and the graphs for reaction 3 for the following questions.
Using the straight line plot makes it possible to determine a parameter which is not given in the data. That parameter is the energy of deactivation, which is found using the following expression: R / (ln(k2) - ln(k1)) x (1/T1 -1/T2)
Examination of the correct answer to the previous question shows that the equality between the rate constants would bring the value of Ea to 0, which corresponds to the most difficult, and therefore the slowest reaction.
Examination of the correct answer to the previous question shows that the equality between the rate constants would bring the value of Ea to 0, which corresponds to the easiest, and therefore the fastest reaction.
Explanation / Answer
The answers to the problem is as given below.
The following statements are true :
(a) True : Determination of the orders and the rate constant of the reaction makes it possible to determine the rate law of the reaction which r = 5000 / [NO] * [H2]^2. The fact the rates of the reaction is correlated to the initial concentrations indicates that the experiment studies the integrated rate law for the reaction between NO and H2.
(b) True : In the expression of the rate law, as the reaction progresses the amounts of NO and H2. Decrease which means that they are the variables of the law, while the rate constant and the reaction orders do not change throughout the reaction, which means that they are the constants of the rate law.
(c) True : Examination of the correct answer to the previous question shows that the equality between the rate constants would bring the value of Ea to 0, which corresponds to the most difficult, and therefore the slowest reaction.
The following statement is False :
(a) False : Using the straight line plot makes it possible to determine a parameter which is not given in the data. That parameter is the energy of deactivation, which is found using the following expression: R / (ln(k2) - ln(k1)) x (1/T1 -1/T2)
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