we start by analyzing the characteristics of a zero-order reaction. The defining feature of zero-order kinetics is that the rate of reaction does not depend on the concentration of the reactant. The rate law is given as: \[ r = k[\text{R}]^0 = k. \] This indicates a constant rate of reaction throughout the process.
Graphical Approach: For a zero-order reaction, the integrated rate equation is: \[ [\text{R}] = [\text{R}_0] - k t, \] where \( [\text{R}_0] \) is the initial concentration, \( k \) is the rate constant, and \( t \) is time. This equation represents a straight-line graph when \( [\text{R}] \) is plotted against \( t \), with: - Slope = \( -k \) (negative value due to the decreasing concentration over time). - Y-intercept = \( [\text{R}_0] \).
Deriving the Correct Plot: To verify the graphical representation, consider the following steps: 1. At \( t = 0 \): \( [\text{R}] = [\text{R}_0] \), which matches the y-intercept. 2. At \( t = \frac{[\text{R}_0]}{k} \): \( [\text{R}] = 0 \), which corresponds to the time at which the reactant is fully consumed. Thus, the plot of \( [\text{R}] \) versus \( t \) will be a straight line with a downward slope, consistent with the equation.
Final Answer: (2)
A(g) $ \rightarrow $ B(g) + C(g) is a first order reaction.
The reaction was started with reactant A only. Which of the following expression is correct for rate constant k ?
Rate law for a reaction between $A$ and $B$ is given by $\mathrm{R}=\mathrm{k}[\mathrm{A}]^{\mathrm{n}}[\mathrm{B}]^{\mathrm{m}}$. If concentration of A is doubled and concentration of B is halved from their initial value, the ratio of new rate of reaction to the initial rate of reaction $\left(\frac{\mathrm{r}_{2}}{\mathrm{r}_{1}}\right)$ is
For $\mathrm{A}_{2}+\mathrm{B}_{2} \rightleftharpoons 2 \mathrm{AB}$ $\mathrm{E}_{\mathrm{a}}$ for forward and backward reaction are 180 and $200 \mathrm{~kJ} \mathrm{~mol}^{-1}$ respectively. If catalyst lowers $\mathrm{E}_{\mathrm{a}}$ for both reaction by $100 \mathrm{~kJ} \mathrm{~mol}^{-1}$. Which of the following statement is correct?
What is the empirical formula of a compound containing 40% sulfur and 60% oxygen by mass?