The rate constant of a zero order reaction is 0.2 mol $d m^{- 3} h^{- 1}$ . If the concentration of the reactant after 30 minutes is 0.5 mol $d m^{- 3}$ . Then its initial concentration would be :-

0.60 mol

d m^{- 3}

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0.15 mol

d m^{- 3}

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0.25 mol

d m^{- 3}

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4.00 mol

d m^{- 3}

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Solution

The correct option is A 0.60 mol $d m^{- 3}$
For zero order reaction : $C_{t}$ = $C_{o}$ - kt
$C_{o}$ : initial concentration
$C_{t}$ : concentration at time "t"
k : rate constant of reaction.
t : convert time in hours as rate constant is in hours
So , $0.5 =$ $C_{o}$ $- (30 / 60) \times 0.2$
$C_{o}$ = 0.6 .
Initial concentration is 0.6 .

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\begin{matrix} Experiment No. & [A] (m o l d m^{- 3}) & [B] (m o l d m^{- 3}) & [C] (m o l d m^{- 3}) & Rate of the reaction (m o l d m^{- 3} s^{- 1}) 1 & 0.2 & 0.1 & 0.1 & 6.0 \times 10^{- 5} 2 & 0.2 & 0.2 & 0.1 & 6.0 \times 10^{- 5} 3 & 0.2 & 0.1 & 0.2 & 1.2 \times 10^{- 4} 4 & 0.3 & 0.1 & 0.1 & 9.0 \times 10^{- 5} \end{matrix}

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Under the same reaction conditions, initial concentration of 1.386 $m o l d m^{- 3}$ of a substance becomes half in 40 s amd 20 s through first order and zero order kinetics respectively. Ratio $(\frac{k_{1}}{k_{0}})$ of the rate constants for first order $(k_{1})$ and zero order $(k_{0})$ of the reaction is:

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The rate constant of a zero order reaction is 0.2 mol dm−3h−1. If the concentration of the reactant after 30 minutes is 0.5 mol dm−3. Then its initial concentration would be :-

The correct option is A 0.60 mol dm−3For zero order reaction : Ct = Co - ktCo : initial concentrationCt : concentration at time "t" k : rate constant of reaction. t : convert time in hours as rate constant is in hoursSo , 0.5= Co −(30/60)×0.2Co = 0.6 .Initial concentration is 0.6 .

The rate constant of a zero order reaction is 0.2 mol $d m^{- 3} h^{- 1}$ . If the concentration of the reactant after 30 minutes is 0.5 mol $d m^{- 3}$ . Then its initial concentration would be :-