The half-life of a zero-order reaction is $1 \text{ hour}$. If the initial concentration of the reactant is $2.0 \text{ mol L}^{-1}$, find the time required to decrease the concentration from $0.50 \text{ mol L}^{-1}$ to $0.25 \text{ mol L}^{-1}$. (in $\text{ hour}$)
- A$0.25$
- B$0.50$
- C$0.75$
- D$1.00$
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Which of the following statements about zero order reaction is not true?
Medium
View SolutionFor 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 $(mol \ L^{-1})$ |
| $0$ | $0.1$ |
| $15$ | $0.05$ |
| $20$ | $0.1 - x$ |
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View SolutionDescribe the nature of the following graphs for a zero-order reaction:
$(i)$ Concentration of reactant $\to$ Time
$(ii)$ Concentration of product $\to$ Time
$(i)$ Concentration of reactant $\to$ Time
$(ii)$ Concentration of product $\to$ Time
Medium
View SolutionThe 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 formation of gas at the surface of tungsten due to adsorption is a reaction of which order?
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