Question

1-The rate constant of a chemical reaction was measured at several temperature values and a plot of ln k (on the y-axis) was plotted against 1/T (on the x-axis, temperature was measured in Kelvin).

If the slope of the plot was -9.21 x 10³ K and the y-intercept was 13.0, what is the activation energy (E_A) of the reaction in kJ mol^-1?

2-In an enzyme-catalyzed reaction, the rate of the reaction depends on which of the following at very low substrate concentrations?

Select one:

Neither enzyme concentration nor substrate concentration

Enzyme concentration but not substrate concentration

Substrate concentration but not enzyme concentration

Both substrate concentration and enzyme concentration

3-The following chemical reaction: A → products shows first order kinetics with respect to A; rate = k[A].

If k = 0.61 x 10^-4 s^-1 and the initial concentration of A is 0.62 mol L^-1, what is the half life of this reaction in minutes?

You have 5 attempts at this question.

Remember: if you want to express an answer in scientific notation, use the letter "E". For example "4.32 x 10⁴" should be entered as "4.32E4".

4-The following chemical reaction: A → products shows first order kinetics with respect to A; rate = k[A].

Assume k = 13.84 x 10^-4 s^-1 .

If the initial concentration of A is 1.19 mol L^-1, what is the concentration of A (in mol L^-1) after 50.2 minutes?

You have 5 attempts at this question.

Remember: if you want to express an answer in scientific notation, use the letter "E". For example "4.32 x 10⁴" should be entered as "4.32E4".

5- Consider the following balanced chemical equation:

H₂O_{2 (aq)} + 3 I^-_(aq) + 2 H⁺_(aq) → I₃^- _(aq) + 2 H₂O _(l)

In the first 22.1 seconds of the reaction, the concentration of H₂O₂ decreased from 1.67 M to 0.56 M.

What is the average reaction rate over this time interval (in mol L^-1 s^-1)?

You have 5 attempts at this question.

Remember: if you want to express an answer in scientific notation, use the letter "E". For example "4.32 x 10⁴" should be entered as "4.32E4".

6-Consider the following balanced chemical reaction:

A + B → C

The following table shows initial reaction rates obtained using different initial concentration of A and B:

Initial [A] (mol L-1)	Initial [B] (mol L-1)	Initial Rate (mol L-1 s-1)
0.202	0.350	0.138
0.202	0.701	0.277
0.604	0.350	0.413
0.604	0.701	0.827

If rate = k[A]^m[B]ⁿ , then m =  -10123 and n =  -10123

7- The following chemical reaction: A → products shows second order kinetics with respect to A; rate = k[A]².

If k = 10.90 x 10^-3 mol^-1 L s^-1 and the initial concentration of A is 0.13 mol L^-1, what is the half life of this reaction in minutes?

You have 5 attempts at this question.

Remember: if you want to express an answer in scientific notation, use the letter "E". For example "4.32 x 10⁴" should be entered as "4.32E4".

8- The following chemical reaction: A → products shows second order kinetics with respect to A; rate = k[A].

Assume k = 2.39 x 10^-5 mol^-1 L s^-1 .

If the initial concentration of A is 0.68 mol L^-1, what is the concentration of A (in mol L^-1) after 8.16 hours?

You have 5 attempts at this question.

Remember: if you want to express an answer in scientific notation, use the letter "E". For example "4.32 x 10⁴" should be entered as "4.32E4".

9- The following chemical reaction: A → products shows zero order kinetics with respect to A; rate = k[A]⁰.

If k = 8.93 x 10^-4 mol L^-1 s^-1 and the initial concentration of A is 0.429 mol L^-1, what is the half life of this reaction in minutes?

You have 5 attempts at this question.

Remember: if you want to express an answer in scientific notation, use the letter "E". For example "4.32 x 10⁴" should be entered as "4.32E4".

10- The following chemical reaction: A → products shows zero order kinetics with respect to A; rate = k[A]⁰.

Assume k = 0.28 x 10^-4 mol L^-1 s^-1 .

If the initial concentration of A was 0.600 mol L^-1 and then decreased to 0.033 mol L^-1 , how much time elapsed in minutes?

You have 5 attempts at this question.

Remember: if you want to express an answer in scientific notation, use the letter "E". For example "4.32 x 10⁴" should be entered as "4.32E4".

Answer 1

Here for first ,second and zero order reaction the rate equation can be written as :

A------> P

[A]t=−kt+[A]_o (first order)

1/[A] = 1/[A]_o +kt (second order)

[A]= [A]_o -kt (zero order)