$A$ person's wound was exposed to some bacteria and then bacteria growth started to happen at the same place. The wound was later treated with some antibacterial medicine and the rate of bacterial decay $(r)$ was found to be proportional to the square of the existing number of bacteria at any instance. Which of the following set of graphs correctly represents the 'before' and 'after' situation of the application of the medicine?
[$Given: N = \text{No. of bacteria}, t = \text{time}$, bacterial growth follows $1^{st}$ order kinetics.]
[$Given: N = \text{No. of bacteria}, t = \text{time}$, bacterial growth follows $1^{st}$ order kinetics.]
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Similar Questions
If the half-life periods of a first-order reaction and a zero-order reaction are equal,then the ratio of the initial rates of the reactions will be .............
Medium
View SolutionMatch the column $I$ with column $II$ :
$a$. Rate constant for first order reaction $i$. $mol \ lit^{-1} \sec^{-1}$ $b$. Molarity $ii$. $\frac{k \times 1000}{M}$ $c$. Rate constant for zero order reaction $iii$. $second^{-1}$ $d$. Limiting molar conductivity $iv$. $\frac{\text{moles of solute}}{\text{Volume of solution (lit)}}$
| $a$. Rate constant for first order reaction | $i$. $mol \ lit^{-1} \sec^{-1}$ |
| $b$. Molarity | $ii$. $\frac{k \times 1000}{M}$ |
| $c$. Rate constant for zero order reaction | $iii$. $second^{-1}$ |
| $d$. Limiting molar conductivity | $iv$. $\frac{\text{moles of solute}}{\text{Volume of solution (lit)}}$ |
Medium
View Solution$t_{100\%}$ is the time required for the $100\%$ completion of the reaction,while $t_{1/2}$ is the time required for $50\%$ of the reaction to be completed. Which of the following options correctly represents the relation between $t_{100\%}$ and $t_{1/2}$ for zero and first-order reactions,respectively?
Half-lives of a first-order and a zero-order reaction are the same. Assume that the initial concentration of the reactant is the same for both reactions,then the ratio of the initial rates of the first-order reaction to that of the zero-order reaction is:
Medium
View SolutionUnder the same reaction conditions,initial concentration of $1.386 \ mol \ dm^{-3}$ of a substance becomes half in $40 \ s$ and $20 \ s$ through first order and zero order kinetics,respectively. The ratio $\left(\frac{k_1}{k_0}\right)$ of the rate constants for first order $\left(k_1\right)$ and zero order $\left(k_0\right)$ of the reactions is:
DifficultIIT 2008
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