Question

The time for half life period of a certain reaction
A → Products is 1 hour. When the initial concentration
of the reactant ‘A’, is 2.0 mol L⁻¹, how much time does it take
for its concentration to come from 0.50 to 0.25 mol L⁻¹ if it is
a zero order reaction ?
(a) 4 h (b) 0.5 h (c) 0.25 h (d) 1 h

Answer 1

Explanation:

hope it helps........ u

Answer 2

The zero order reaction takes (c) 0.25 h to get reduced from 0.50 to 0.25 mol L⁻¹.

Given:

$[A_0]$ = 2.0 M

$t_\frac{1}{2}$ = 1 hr

k = 1

To find:

t = ?

Formula to be used:

$k = \frac{x}{t}$

Calculation:

For a zero order reaction,

$k = \frac{x}{t}$ ......... (1)

Where

x - Amount of reactant decomposed

For a zero order reaction

$k=\frac{[A_0]}{2t_\frac{1}{2} }$

From equation (1)

$k = \frac{x}{t}$

$k\times t=x$

$t=\frac{x}{k}$

Substituting the values, it gives

$t=\frac{x}{k}$

$t=\frac{0.25}{1}$

t = 0.25 h

Conclusion:

Thus it is inferred that for reduction of concentration of reactant from 0.50 to 0.25 mol L⁻¹ it takes 0.25 h.

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