According to the kinetic molecular theory, the pressure of a gas in a container will increase if the
es (1)
A)
number of collisions with the container wall increases.
number of moles of the gas decreases.
temperature of the gas decreases
D
v olume of the container increases.
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According to the kinetic molecular theory, the pressure of a gas in a container will increase if the "number of collisions with the container wall increases".

Option: A

Explanation:

Pressure is characterized as force acting by area per unit. It is triggered by gas molecules bombarding on the container walls. Kinetic molecular theory suggests that gases are made up of large numbers of small particles with continuous movement. Here there are elastic collisions between gas particles and between particles and container walls. There are no forces of attraction among them because of the large spaces between the gas particles. The gas temperature relies on the particle's average kinetic energy.

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

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