The rate constant of a zero-order reaction is $0.2 \ mol \ m^{-3} \ h^{-1}$. If the concentration of the reactant after $30 \ minutes$ is $0.05 \ mol \ m^{-3}$,then its initial concentration will be ....... $mol \ m^{-3}$.
- A$0.15$
- B$1.05$
- C$0.25$
- D$4.00$
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Similar Questions
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 2017
View SolutionFor a zero-order reaction,the correct expression for rate constant $(k)$ at half-life time $(t_{1/2})$ is ($[R_0] =$ initial concentration of reactant).
For a zero order reaction,which of the following statements is false?
Medium
View SolutionWhich among the following is an example of a zero order reaction?
Calculate the rate constant of a zero order reaction if it is $90 \%$ completed in $90 \ s$.
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