The rate constant of the reaction $A \rightarrow B$ is $0.6 \times 10^{-3} \, mol \, L^{-1} \, s^{-1}.$ If the concentration of $A$ is $5 \, M,$ then the concentration of $B$ after $20$ minutes is ......... $M.$
- A$3.60$
- B$0.36$
- C$0.72$
- D$1.08$
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For the reaction $A \longrightarrow 3 B$,the rate is given by $rate = k[A]^0$. Based on the data provided in the table,what is the concentration of the product $B$ (in $mol \ L^{-1}$) after $20 \ s$?
Time $(s)$ Concentration of the reactant $(mol \ L^{-1})$ $0$ $0.1$ $15$ $0.05$ $20$ $0.1 - x$
| Time $(s)$ | Concentration of the reactant $(mol \ L^{-1})$ |
| $0$ | $0.1$ |
| $15$ | $0.05$ |
| $20$ | $0.1 - x$ |
DifficultAP EAMCET 2022
View SolutionWhich of the following is the slope of the graph of $[A]_{t}$ versus time for a zero order reaction?
The rate constant of a zero order reaction is $2.0 \times 10^{-2} \ mol \ L^{-1} \ s^{-1}$. If the concentration of the reactant after $25 \ s$ is $0.5 \ M$,then find the initial concentration of the reactant. (in $M$)
The plot of concentration of a reactant versus time for a chemical reaction is shown below. The order of this reaction with respect to the reactant is
MediumKVPY 2019
View SolutionWhich of the following plots is correct for a zero-order reaction?
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