Question

Which of the following plots is (are) correct for the given reaction? ([P]₀ is the initial concentration of P)

• A.
• B.

  

• C.

  

• D.

  

Answer 1

The correct option is A

In the given plots option A is correct for the given

This is such a first-order reaction, that the rate of the reaction may be approximately equal to one of the reactants' concentrations. In a first-order reaction, the rate of reaction is equivalent to the initial concentration scaled by the first power. The chemical tends to be unchanged by the number of other reactants. As a function, the order of a first-order interaction is always one.

The plot which is correct is option A

Because for a first-order reaction $t_{1/2}=\frac{0.693}{k}$

As a function, their half-life is untouched by the initial concentration.

The plot which is incorrect is options B & D

For the first-order reaction,
$(r)=k[(C{H}_3{)}_{3}C-Br]$ ;
$\ln \left(\frac{P_0}{P}\right)=kt$

or $\ln \left(\frac{P}{P_0}\right)=-kt$
As an outcome, plots (b) and (d) are misleading.

The plot which is incorrect is option C

For the first-order reaction,
Q = [P₀](1 $-$ e^kt)
Or $\frac{[Q]}{[P_0]}=(1-e^{kt})$
Hence, plot(c) is inaccurate.

Conclusion

On the whole option, A is the correct answer