Question

what can you conclude from the graph?
the reaction that causes a firework to explode requires more energy to start, and occurs more rapidly than the
reaction that causes a candle to burn.
the reaction that causes a firework to explode requires more energy to start, and occurs less rapidly than the
reaction that causes a candle to burn.
the reaction that causes a firework to explode requires less energy to start, and occurs less rapidly than the
reaction that causes a candle to burn.
the reaction that causes a firework to explode requires less energy to start, and occurs more rapidly than the
reaction that causes a candle to burn.

Explanation:

Step1: Analyze energy - start relationship

In chemical reactions, the energy required to start a reaction is related to the activation energy. A reaction with higher activation energy (more energy to start) generally occurs more slowly. A reaction with lower activation energy (less energy to start) occurs more rapidly.

Step2: Analyze the graph

Looking at the graph, the blue line (assuming it represents the candle - burning reaction) has a lower energy increase initially (lower activation energy). The orange line (assuming it represents the firework - exploding reaction) has a higher energy increase initially (higher activation energy).
Since the candle - burning reaction (blue line) has lower activation energy (less energy to start), and the firework - exploding reaction (orange line) has higher activation energy (more energy to start). Also, reactions with lower activation energy occur more rapidly.

Answer:

The reaction that causes a candle to burn requires less energy to start, and occurs more rapidly than the reaction that causes a firework to explode.