The graph shows the distribution of energy in the particles of two gas samples at different temperatures, T1 and T2. A, B, and C

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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.
A graph is shown with two inverted graph curves running close to each other. One of the curves labeled T1 is slightly more spread out than the other labeled T2. The x axis of the graph has the title Kinetic Energy. The y axis of the graph has the title Number of Particles. A vertical line perpendicular to the x axis is shown. This vertical line is labeled Activation Energy. A point labeled B is shown on the right hand side of the vertical line. A point labeled A is shown in the lower left side of the vertical line. A particle labeled C is shown in the upper left side of the vertical line.

Based on the graph, which of the following statements is likely to be true?
Particle A and C are more likely to participate in the reaction than particle B.
Most of the particles of the two gases have very high speeds.
A fewer number of particles of gas at T1 are likely to participate in the reaction than the gas at T2.
The average speed of gas particles at T2 is lower than the average speed of gas particles at T1.

Chemistry

1 answer:

lions [2.9K] · Answer 1 · 2026-02-25T02:41:17+03:00

Answer:

The average velocity of gas molecules at T₂ is less than the average velocity of gas molecules at T₁.

Explanation:

Particles A and C appear aligned vertically, suggesting they share the same kinetic energy. Given that both are positioned to the left of particle B, it indicates that A and C possess lesser kinetic energy than B.

The likelihood of a particle engaging in a reaction is directly proportional to its kinetic energy, meaning that particle B is more prone to react compared to A and C. Thus, the first statement is incorrect.

The graph resembles a bell curve, demonstrating a mixture of many molecules with low and high kinetic energy. Therefore, one cannot conclude that most particles in both gases have high velocities. As a result, the second statement is also incorrect.

Examining the higher kinetic energy values (to the right of the curve), the line for T₁ exceeds that for T₂, indicating that more molecules possess high kinetic energy at T₁ compared to T₂.

Conversely, for lower kinetic energy values (to the left of the curve), T₂'s line is above T₁'s, which implies that at T₂ there are more molecules with low kinetic energy than at T₁.

Thus, the observations from the previous two paragraphs suggest that the average kinetic energy of gas particles at T₂ is lower than the average kinetic energy of particles at T₁.

Since average speed is proportional to the square root of temperature, the relationship that applies to average kinetic energy equally pertains to average speed, leading us to conclude that the last statement holds true: "The average speed of gas particles at T₂ is lower than at T₁.".

Additionally, given that there are more gas molecules at T₁ with higher kinetic energy compared to those at T₂, it indicates that gas particles at T₁ are more likely to react than those at T₂, marking the third statement as incorrect.