The graph below compares the rates of reaction of a burning candle and an exploding firework.

Comparing Chemical Reactions
A graph has time on the horizontal axis and concentration of reactants on the vertical axis. For an exploding firework, the concentration starts high, increases slightly and then decreases rapidly. For a burning candle the concentration starts high, increases more than the firework, and then decreases rapidly. The concentration for the burning candle is higher than the firework at all timepoints.

What can you conclude from the graph?
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.
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 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 more energy to start, and occurs more rapidly than the reaction that causes a candle to burn.

The speed of a chemical reaction and the amount of energy required for this reaction is directly linked to the concentration of reagents present in the system. With that, we can say that the higher the concentration of reagents, the faster the chemical reaction will be due to the greater probability of collision between its molecules.

Although the reaction that causes a candle to burn has more reactants than the reaction that causes the fireworks to explode, the latter requires less energy to start. This makes the molecules of the reagents stir faster and collide more efficiently, making the reaction happen much faster.

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

pstnonsonjoku pstnonsonjoku · Answer 2 · 2021-10-31T06:52:45+01:00

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 rate of reaction refers to the ease with which reactants are converted to products. The higher the rate of reaction, the faster reactants are converted into products.

The activation energy is the energy required for reactants to be converted into products. It is an energy barrier that separates reactants and products.

From the description of the graphs, we are told that the reaction that causes the explosion of firework starts at high concentration, initially increases slightly then decreases rapidly. The fact that it initially increased slightly before decreasing rapidly implies that the high energy required for the reaction to start is high.

On the other hand, the reaction for the candle to burn starts at high concentration, increases more than the firework, and then decreases rapidly because the reaction requires a lesser energy to commence than the reaction for the burning of candle.

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