Question

In a given graph of zero order reaction, the slope and intercept are:

• A. Slope = k, Intercept = [R]$_0$
• B. Slope = -k, Intercept = [R]$_0$
• C. Slope = k/2.303, Intercept = ln[R]$_0$
• D. Slope = -k/2.303, Intercept = ln A

Hint:

In zero-order reactions, a plot of concentration vs. time gives a straight line with a slope of \(-k\) and an intercept of \([R]_0\).

Answer 1

The Correct Option is B

For a zero-order reaction, the integrated rate law is given by: \[ [R] = [R]_0 - kt \] Where:
- \([R]\) is the concentration of reactant at time \(t\),
- \([R]_0\) is the initial concentration,
- \(k\) is the rate constant,
- \(t\) is time.
When plotted as \([R]\) vs. \(t\), the slope of the graph is \(-k\), and the y-intercept is \([R]_0\).

Step 1: The slope of the line is equal to \(-k\) because of the negative relationship between concentration and time.
Step 2: The y-intercept is the initial concentration of the reactant.