Question

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Please answer this question with proper explanation.

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Answer 1

Answer:

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100% it is correct

Answer 2

Question :-

Given above ↑

Explanation :-

(a) Write the rate law for the reaction

$\leadsto \sf let \: rate \: = k {[A]}^{x} {[B]}^{y}$

• . • initial rate formation is given in the table hence rate law is -

$\boxed{.} \: \sf 1.5 \times {10}^{ - 3} mol \: {L}^{ - 1} {min}^{ - 1} = k {(0.1)}^{x} {(0.1)}^{y} \\ \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: .....(1) \\ \\ \boxed{.} \sf3 \times {10}^{ - 3} mol \: {L}^{ - 1} {min}^{ - 1} = k {(0.2)}^{x} {(0.2)}^{y} \: \\ \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: ......(2)\: \\ \boxed{.} \sf6 \times {10}^{ - 3} mol \: {L}^{ - 1} {min}^{ - 1} = k {(0.2)}^{x} {(0.4)}^{y} \: \\ \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: ..... (3)$

now (3) divided by (2)

$\leadsto \sf\frac{6 \times {10}^{ - 3} }{3 \times {10}^{ - 3} } = \frac{k {(0.2)}^{x} {(0.4)}^{y} }{k {(0.2)}^{x} {(0.2)}^{y} } \\ \\ \leadsto \sf 2 = {( \frac{0.4}{0.2} )}^{y} \\ \\ \leadsto \sf \: 2 = {2}^{y} \implies \boxed{ \sf y = 1}$

Now (2) divided by (1)

$\leadsto \sf \frac{3 \times {10}^{ - 3} }{1.5 \times {10}^{ - 3} } = \frac{k {(0.2)}^{x} {(0.2)}^{y} }{k {(0.1)}^{x} {(0.1)}^{y} } \\ \\ \leadsto \sf 2 = { (\frac{0.2}{0.1}) }^{x} {( \frac{0.2}{0.1} )}^{y} \\ \\ \leadsto \sf 2 = {2}^{ x + y} \: \: \because \: y = 1 \\ \\ \leadsto \sf 2 = {2}^{x} \: 2 \\ \\ \leadsto \boxed{ \sf \: x = 0}$

Hence rate is

$\leadsto \sf \boxed{ \sf Rate \: = k {[A]}^{0} {[B]}^{1} } \\ or \\ \leadsto \boxed{ \sf Rate \: = k {[B]}^{1} }$

\_________________/

(b) Calculate the value of rate constant -

$\leadsto \: K = \frac{Rate}{[B] \: \: } \\ \\ \leadsto \sf K = \frac{1.5 \times {10}^{ - 3} mol \: {L}^{ - 1} {min}^{ - 1} \: }{0.1mol \: {L}^{ - 1} \: } \\ \\ \leadsto \boxed{ \sf K = 15 \times {10}^{ - 3} { min}^{ - 1} } \\ or \\ \leadsto \: \boxed{ \sf K = 1.5 \times {10}^{ - 2} { min}^{ - 1} } \:$

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(c) which of the following possible reaction mechanism is consistent with the rate law

Answer :-

(ii)

♣ B → C + E ( slow step )

♣ A + E→ F ( fast step )