The graph shows the distribution of energy in the particles of two gas samples at different temperatures, t1 and t2. a, b, and c represent individual particles.

based on the graph, which of the following statements is likely to be true?

particle b is more likely to participate in the reaction than particle a.
particle c is more likely to participate in the reaction than particle b.
most of the gas particles have either very high or very low kinetic energies.
more gas particles participate in the reaction at t2 than at t1.

Particle B is more likely to participate in the reaction than particle A

Explanation:

Activation energy is defined as an energy barrier that needs to be overcome in order for a reaction to proceed. That is, for a reaction to take place, the minimum energy that particles should possess would be equal to the activation energy.

Notice that particles B have a higher kinetic energy than the remaining particles, besides, this energy is greater than the activation energy. This implies that particles B are much more likely to participate in a reaction.

Particle B is more likely to participate in the reaction than particle A.

Explanation:

took test

i know insulin is primary but i dont know the others im sorry

explanation:

the answer is:  

line graphs show patterns in data with variables that change over time; whereas, circle graphs show data as parts out of a whole (such as out of 100%).