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Consider the reaction A + B ? products From the following data obtained at a certain…

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Question “Consider the reaction A + B ? products From the following data obtained at a certain…”

Consider the reaction A + B ? products

From the following data obtained at a certain temperature,
determine the rate law, the order of the reaction, and calculate
the rate constant k.

Experiment 1: [A] = 1.50 M; [B] = 1.50 M; Initial Rate = 3.20 x
10-1 M/s

Experiment 2: [A] = 1.50 M; [B] = 2.50 M; Initial Rate = 3.20 x
10-1 M/s

Experiment 3: [A] = 3.00 M; [B] = 1.50 M; Initial Rate = 6.40 x
10-1 M/s

Please explain to me how you got the answer step by step ><
Thank you!

A. Rate = k[A][B]

order of reaction = 2

k = 0.142 s-1

B.Rate = k[A]

order of reaction = 1

k = 0.213 s-1

C. Rate = k[A]2

order of reaction = 2

k = 0.142 s-1

D. Rate = k[B]

order of reaction = 1

k = 0.213 s-1

Answer

Concepts and Reason

Rate at which the reaction occurs:Rate refers to the change in concentration or product concentration per unit of time.


Rate=AIConcentration] At Atis the change in time


The temperature, pressure and concentration of reactants or products affect the rate of reaction. It is dependent on temperature. Only the Arrhenius equation relates temperature and rate in chemical kinetics.

The order of the reaction is dependent on the n-value. Here, n is the sum power of the stoichiometry coefficients.

Rate constant : The rate constant (k), is the proportionality constant for a reaction that depends on temperature.

Rate law expression The rate law expression refers to the rate of reaction, the rate constant and the concentration of reactant or product.

Fundamentals

The following is a rate law:


aА+bВ- — ></figure><p>sS @dD rate k[AJ] [B]</a><br /> </a></p></div><p> That is why</p><p> <a href=

Consider the reaction A + B ? products From the following data obtained at a certain...

Let’s get it!

Experiments

[A]

M

[B

M

M/s Initial Rate

1


1.50 M


1.50 M

3.20x10 M/s

2


1.50 M



2.50 M



3.20x10 M/s


3


3.00 M



1.50 M



6.40x10 M/s


rate k[A[B

.

Take experiment (1) and (2)

Divide (1) by (2)


k[A][B]* k[A[B 3.20x10 M/s [1.50] [1.50]| 3.20*10M/s 1.50] [2.50]* [1502.50 l= [0.6


b 0

Divide (1) by (3)


k[A] [B] k[AJ[BJ 3.20x10 M/s [1.50] [1.50]| 6.40x10 M/s 3.00r [1.50]* 0.5= [0.5]


а 31



Rate k[A] B]J



Rate k[A

————————–(1)

The rate of the given reaction does not depend on the

В

concentration, so the options A and B are incorrect.


А. Rate k A][B] order of reaction =2 k 0.142 s



D. order of reaction =1 Rate k [B] k 0.213 s


The order of the reaction does not equal two. Therefore, the option C is incorrect.


С. Rate kA] order of reaction = 2 k 0.142 s


In rate expression, substitute the concentration and rate

Rate k[A]

—————————-(1)



Order of reaction = 1





rate k [A] 6.40x10 M/s 3.00M k 0.213s



The best option is therefore B

Ans:


Rate law, rate order and rate constant were identified. They are highlighted in



A. Rate k[A][B],order of reaction-2,k =0.142s. B.Rate k[A],order of reaction =1,k = 0.213 s1. C. Rate k[AT,0rder of reaction



Conclusion

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