For a first order reaction,the concentration of reactant decreases from $0.2 \ M$ to $0.1 \ M$ in $100 \ minutes$. What is the rate constant of the reaction?
- A$6.93 \ min^{-1}$
- B$69.3 \ min^{-1}$
- C$6.93 \times 10^{-3} \ min^{-1}$
- D$144.3 \ min^{-1}$
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Similar Questions
If the concentration is expressed in moles per litre,the unit of the rate constant for a first order reaction is
Easy
View Solution$A \rightarrow$ products is a first-order reaction. The following data is obtained for this reaction at $T \ K$. The value of $x : y$ is:
Rate $(\text{mol } L^{-1} \ \text{min}^{-1})$ $[A]$ $0.2$ $0.02 \ M$ $0.4$ $x \ M$ $1.0$ $y \ M$
| Rate $(\text{mol } L^{-1} \ \text{min}^{-1})$ | $[A]$ |
|---|---|
| $0.2$ | $0.02 \ M$ |
| $0.4$ | $x \ M$ |
| $1.0$ | $y \ M$ |
For a first order gas phase reaction:
$A_{(g)} \rightarrow 2 B_{(g)} + C_{(g)}$
Let $P_0$ be the initial pressure of $A$ and $P_t$ be the total pressure at time $t$. The integrated rate equation is:
$A_{(g)} \rightarrow 2 B_{(g)} + C_{(g)}$
Let $P_0$ be the initial pressure of $A$ and $P_t$ be the total pressure at time $t$. The integrated rate equation is:
DifficultAIIMS 2019
View SolutionIn a first order reaction,$60 \%$ of the reactant converts into product in $45 \ minutes$. Calculate the rate constant of the reaction.
After how many seconds will the concentration of the reactants in a first order reaction be halved,if the decay constant is $1.155 \times 10^{-3} \, \sec^{-1}$?
MediumAIPMT 2000
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