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How does the pressure of a gas change if you increase volume?
If you increase the volume of the container, and not the gas itself, then the pressure decreases. If you increase the volume of the gas, and not the container, then the pressure increases.
Explain why increasing the temperature of a gas in a close the rigid container causes the pressure in the container to increase?
If temperature increases, either the volume or the pressure must increase. Since you have limited the volume by closing the container, pressure must increase.
A student is monitoring the pressure of a gas in a rigid container. The amount of gas particles and the volume of the container are held constant. How will the pressure be affected if the container is?
If the container is heated, the kinetic energy of the gas particles will increase, causing them to move faster and collide more frequently with the container walls. This increase in collisions will lead to a higher pressure within the container.
What will happen to the pressure inside the container if the volume of a container of gas is reduced?
If the volume of a container of gas is reduced, the pressure inside the container will increase. This is because reducing the volume decreases the amount of space the gas molecules have to move around, leading to them colliding more frequently with the walls of the container, thus increasing the pressure.
When the temperature of a gas increases does the volume of the gas increase in a rigid steel container?
No, because the gas is in a rigid steel container, its volume cannot increase as the temperature increases (assuming the steel does not deform). Instead, the pressure of the gas inside the container will increase. Of course, if the pressure is high enough, the container will explode, lowering the pressure and causing the gas to expand.
How does the pressure of a container change as the volume is changed?
According to Boyle's Law, the pressure of a gas in a container is inversely proportional to its volume when temperature is constant. This means that as the volume of the container decreases, the pressure of the gas inside will increase, and vice versa.
If the volume of a container of air is reduced?
If the volume of a container of air is reduced, the pressure of the air inside the container will increase. This is because the volume and pressure of a gas are inversely proportional according to Boyle's Law. The particles inside the container will collide more frequently with the walls, leading to an increase in pressure.
What would the effect on temperature and volume be if you changed the number of moles of gas in a container?
In a container the volume remain constant but the pressure increase.
What will the pressure inside the container become if the piston is moved to the 1.80 L rm L mark while the temperature of the gas is kept constant?
This problem can be solved with the ideal gas law. The original pressure and volume of the container are proportional the final pressure and volume of the container. The original pressure was 1 atmosphere and the original volume was 1 liter. If the final volume is 1.8 liters, then the final pressure is 0.55 atmospheres.
How will decreasing the volume of the container shift the equilibrium?
Decreasing the volume of a container will shift the equilibrium towards the side with fewer gas molecules to increase pressure.
Raising temperature of a gas fixed volume container will change?
The pressure of the gas inside the container will increase due to the increased kinetic energy of the gas molecules. This is described by the ideal gas law, PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the gas constant, and T is temperature.
What effect does an increase in temperature have on a gas's volume and pressure?
As indicated by the Ideal Gas Laws, increasing temperature will tend to increase both volume and pressure. Of course, volume can't always increase, that depends upon the flexibility or inflexibility of the container that the gas is in, and if the volume does increase that will counteract the increase in pressure that would otherwise have happened. Temperature, pressure, and volume are all interconnected in a gas.
