A sample of a gas is in a sealed container. The pressure of the gas is 565 torr , and the temperature is 27 ∘C . If the temperature changes to 71 ∘C with no change in volume or amount of gas, what is the new pressure, P2, of the gas inside the container?

P₂ = 647 torr

Explanation:

Given data:

Initial pressure = 565 torr

Initial temperature = 27°C

Final temperature = 71°C

Final pressure = ?

Solution:

Initial temperature = 27°C (27+273 = 300 K)

Final temperature = 71°C (71+273 = 344 K)

According to Gay-Lussac Law,

The pressure of given amount of a gas is directly proportional to its temperature at constant volume and number of moles.

Mathematical relationship:

P₁/T₁ = P₂/T₂

Now we will put the values in formula:

565 torr / 300K = P₂/344 K

P₂ = 565 torr × 344 K / 300 K

P₂ = 194360 torr. K /293 K

P₂ = 647 torr

both adhesion and cohesion are attractions.

they are different in that adhesion is the force of attraction between the molecules of two different substances, whereas cohesion is the force of attraction between molecules of the same substance.

possible examples include capillary action, in which the adhesion between water and glass causes the water to rise in a narrow tube against the force of gravity.

because of hydrogen bonding, water is extremely cohesive.

this causes molecules on the surface of water to be drawn inward, which is why drops of water form beads on smooth surfaces.

hope this .

the answer is barium and copper bromide