$A$ 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
For the following parallel chain reaction,what will be the value of the overall half-life of $A$ in minutes?
Given that $\frac{[B]_t}{[C]_t} = \frac{16}{9}$
$A \xrightarrow{k_1 = 2 \times 10^{-3} \ s^{-1}} 4B$
$A \xrightarrow{k_2} C$
Given that $\frac{[B]_t}{[C]_t} = \frac{16}{9}$
$A \xrightarrow{k_1 = 2 \times 10^{-3} \ s^{-1}} 4B$
$A \xrightarrow{k_2} C$
Match 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$A$ substance $S$ undergoes two reactions under similar reaction conditions:
$\mathop S\limits_{(2.0 \ M)} \xrightarrow{K_0} X$ (zero order)
$\mathop S\limits_{(2.0 \ M)} \xrightarrow{K_2} Y$ (second order)
The time taken for the concentration of $S$ to become half is $40 \ s$ and $10 \ s$ for the zero-order and second-order reactions,respectively. What is the value of the ratio $K_0 / K_2$?
$\mathop S\limits_{(2.0 \ M)} \xrightarrow{K_0} X$ (zero order)
$\mathop S\limits_{(2.0 \ M)} \xrightarrow{K_2} Y$ (second order)
The time taken for the concentration of $S$ to become half is $40 \ s$ and $10 \ s$ for the zero-order and second-order reactions,respectively. What is the value of the ratio $K_0 / K_2$?
Medium
View SolutionFor a first order reaction,which of the following statements is correct?
DifficultIIT 1998
View SolutionThe temperature coefficient for a reaction in which food deteriorates is $2$. Then food deteriorates ...... times as rapidly at $25\,^oC$ as it does at $5\,^oC$.
Medium
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