Chemical Kinetics

It decreases the rate by increasing the activation energy.

It has no effect on the rate unless the temperature is changed.

It increases the rate because the particles have higher average kinetic energy.

It increases the rate because there are more particles per unit volume, leading to more frequent collisions.

Interval A

Interval B

Interval C

Interval D

Particles must have identical mass and high velocity.

Particles must collide in the gaseous state and at high pressure.

Particles must collide with sufficient kinetic energy and the correct mutual orientation.

Particles must collide with low potential energy and high frequency.

The rate triples

The rate increases by a factor of nine

The rate decreases by a factor of three

The rate remains unchanged

$Rate = k[NO_2]^2[F_2]$

$Rate = k[NO_2][F_2]$

$Rate = k[F][NO_2]$

$Rate = k[NO_2F][F]$

1

2

3

4

$J \cdot K^{-1} \cdot mol^{-1}$

$mol \cdot dm^{-3} \cdot s^{-1}$

$kJ \cdot mol^{-1}$

$s^{-1}$

The fraction of molecules with energy greater than the activation energy.

The rate constant at $273\ K$.

The ratio of the activation energy to the gas constant.

The frequency of collisions with the correct orientation.

$E_a$ decreases and $\Delta H$ remains constant.

$E_a$ decreases and $\Delta H$ decreases.

$E_a$ increases and $\Delta H$ remains constant.

$E_a$ remains constant and $\Delta H$ decreases.