Question

For a zero order reaction,
K = 1 x 10-3 mol L-1 s-1
If initial concentration of the reactant is
1.0 mol L-1, the concentration after 10 minutes
would be
(1) 1 x 10-2 mol L-1
(2) 0.6 mol L-1
(3) 0.4 mol L-1
(4) 1.0 mol L-1.


GUYS PLEASE SOLVE THIS QUESTION..... ​

Answer 1

Answer:(3)

Explanation:

Follow the eqn of zero order reaction... ans is in the attachment.

Answer 2

Answer:

For zero order reaction, the concentration of reactant after 10 minutes will be equal to 0.4molL⁻¹.

Therefore, option (3) is correct.

Explanation:

For zero order reaction,

Consider that the initial concentration of the reactant is [A₀]

Concentration of reactants left after time t will be $[A_{t}]$

We know that for the zero order reaction:-

$k=\frac{[A_{o}]-[A_{t}]}{t}$                                                        

$kt=[A_{o}]-[A_{t}]$

$[A_{t}]=[A_{o}]-kt$                                              ....................(1)

Given, the value of rate constant, $k=1*10^{-3}molL^{-1}s^{-1}$

The initial concentration of the reactant $[A_{o}]=1.0mloL^{-1}$

Time,  t = 10min = 600sec

Put the value of [A₀], k and t in equation (1);

$[A_{t}]=1molL^{-1}-(1*10^{-3}molL^{-1}s^{-1})(600s)$

$[A_{t}]=(1-0.6)molL^{-1}$

$[A_{t}]=0.4mloL^{-1}$

Therefore, for the given zero order reaction the concentration of reactants after 10 minutes would be equal to 0.4molL⁻¹.