1. collisions of helium atoms with the walls of a closed container cause (1 point) condensation. gas pressure. a decrease in volume. an overall loss of energy. 2. which of the following factors affects the pressure of an enclosed gas? (1 point) temperature volume number of particles all of the above 3. the temperature and volume in a closed container of gas remain constant. if the number of particles of gas is increased, what will happen to the gas pressure? (1 point) it will increase. it will decrease. it will remain constant. you cannot predict it. 4. the volume of a gas is directly proportional to its temperature if the pressure and the number of particles is constant. this is a statement of which law? (1 point) boyle’s law bose’s law einstein’s law charles’ law 5. if the volume of a cylinder is reduced from 8.0 liters to 4.0 liters,

1) Answer is: gas pressure.

The pressure of a gas is the force that the gas exerts on the walls of its closed container.

More collisions of helium atoms with the walls of a closed container, higher the pressure.

Presure also depands on number of helium atoms, temperature and volume of container.

Manometer is a device to measure pressures.

2) Answer is: all of the above.

Boyle's Law: the pressure volume law - volume of a given amount of gas held varies inversely with the applied pressure when the temperature and mass are constant.

When volume goes up, pressure goes down.

Gay-Lussac's Law: the pressure of a given amount of gas held at constant volume is directly proportional to the Kelvin temperature.

As the temperature goes up, the pressure also goes up and vice-versa.

3) Answer is: It will increase.

According to ideal gas law, more gas particles, higher pressure.

An ideal gas is:

1) made up of molecules which are in constant random motion in straight lines.  

2) all collisions are perfectly elastic, there is no loss of kinetic energy during the collision.

3) follows ideal gas law: p·V = n·R·T.

4) the gas particles have negligible volume.

4) Answer is: Charles' Law.

Charles' Law (The Temperature-Volume Law) - the volume of a given amount of gas held at constant pressure is directly proportional to the Kelvin temperature:  

V₁/T₁ = V₂/T₂.  

When temperature goes up, the volume also goes up.  

For example:

V₁(gas) = 2240.0 L; initial volume.

T₁(gas) = 373 K; initial temperature.

T₂(gas) = 273 K; final temperature.

V₂(gas) = ?

2240 L/373 K = V₂/273 K.

V₂ = 1639.46 L.

5) Answer is: 140 kilopascals.

Boyle's Law (the pressure volume law): volume of a given amount of gas held at constant temperature varies inversely with the applied pressure when the temperature and mass are constant.  

p₁V₁ = p₂V₂ (the product of the initial volume and pressure is equal to the product of the volume and pressure after a change).

70 kPa · 8.0 L = p₂ · 4.0 L.  

p₂ = 70 kPa · 8.0 L / 4.0 L.  

p₂ = 140 kPa.

When pressure goes up, volume goes down.  

When volume goes up, pressure goes down.  

1) The pressure of a gas is due to collision of gas particles with the wall of container. Thus

Collisions of helium atoms with the walls of a closed container cause gas pressure

2) The pressure is related to

a) volume : inversely proportional [as explained by Boyel's law]

b) Temperature

c) number of particles

Thus answer is all of the above

3) The ideal gas equation is

PV = nRT

Where

P = Pressure of gas

V = volume of gas

n = moles of gas

T = temperature

R = gas constant

Now as we are keeping T and V constant and increasing the number of molecules it will increase the pressure

It will increase

4) Charle's Law : at constant pressure and constant number of molecules the volume of a gas is directly proportional to its temperature.

i do not get it   at all

it is the most commonly accepted one