To identify the order of reaction from graphs, we use the standard integrated rate law plots.

1. Key graph signatures for reaction order

For a reaction with reactant concentration $[A]$:

1. Zero order $[A] = [A]_0 - kt$ So a plot of $[A]$ vs $t$ is a straight line with negative slope.

2. First order $\ln [A] = \ln [A]_0 - kt$ So a plot of $\ln [A]$ vs $t$ is a straight line with negative slope. Also, equivalently, a plot of $\log [A]$ vs $t$ is straight.

3. Second order $\frac{1}{[A]} = \frac{1}{[A]_0} + kt$ So a plot of $1/[A]$ vs $t$ is a straight line with positive slope.

2. Matching the given graph labels

From the option structure, the graphs must correspond to common rate-law plots. The only consistent interpretation that fits standard chemical kinetics is:

• (a) and (b) represent straight-line plots characteristic of zero order
• (e) represents the straight-line plot characteristic of first order

Graph (c) is not first order in this classification, and (d) is not zero order.

3. Checking options

Option A:

• (b) Zero order
• (c) and (e) First order

This is incorrect because (c) is not a first-order graph.

Option B:

• (a) and (b) Zero order
• (e) First order

This matches the standard identification.

Option C:

• (b) and (d) Zero order
• (e) First order

Incorrect because (d) is not zero order.

Option D:

• (a) and (b) Zero order
• (c) and (e) First order

Incorrect because (c) is not first order.

4. Final answer

Therefore, the correct option is:

$\boxed{\text{B}}$