Question

The rate constant for a particular zero-order reaction is 0.075 M s^-1. If the initial concentration of reactant is 0.537 M it takes _____ s for the concentration to decrease to 0.100 M. A) 5.8 B) -5.8 C) -0.047 D) 7.2 E) 0.040

Answer 1

Answer:

A) 5.8

Explanation:

Integrated rate law for zero order kinetic is:

$[A_t] = [A_0] -kt$

Where, $[A_t]$ is the final concentration  = 0.100 M

$[A_0]$ is the initial concentration  = 0.537 M

k is the rate constant = 0.075 M s⁻¹

For 90% completion, 10% is left. so,

Applying in the values in the above equation as:-

$0.100 = 0.537-0.075\times t$

t = 5.8 seconds

Answer 2

The time for the consumption of reactant from 0.537 M to 0.1 M has been 5.8 s. Thus, option B is correct.

The rate of reaction has been defined as the time taken for the formation of the product concerning the reactants. The zero-order kinetics implies the rate of the reaction has been independent of the reactant concentration.

The integrated zero order rate law has been given by:

$A_t=-kt\;+\;A_o$

Where, the final concentration of reactant, $A_t=0.100\;\text M$

The initial concentration of reactant, $A_0=0.537\;\rm M$

The rate constant for the reaction, $k=0.075\;\rm Ms^-^1$

Substituting the values for calculating time, (t):

$\rm 0.1\;M=-0.075\;Ms^-^1\;\textit t\;+\;0.537\;M\\\rm 0.1\;M\;-\;0.537\;M=-0.075\;Ms^-^1\;\textit t\\\textit t=5.8\;s$

The time for the consumption of reactant from 0.537 M to 0.1 M has been 5.8 s. Thus, option B is correct.

For more information about zero-order reaction, refer to the link:

https://brainly.com/question/8139015