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A gas sample is held at constant temperature. What happens to the pressure of the sample if the volume is doubled and the number of molecules is doubled?
If the volume is doubled and the number of molecules is doubled while the temperature is held constant, the pressure of the gas sample will remain the same. This is because both the volume and the number of molecules increased by the same factor, resulting in no net change in pressure according to the ideal gas law.
Imagine that bubbles begin to form a sample of liquid but the temperature did not change.what must have happened to cause this change?
The decrease in pressure caused the bubbles to form in the liquid sample without changing the temperature. This could occur, for example, if the liquid was moved to a region of lower pressure, releasing dissolved gases as bubbles.
What temperature change would cause a sample of an ideal gas to double in volume while the pressure was held constant?
If the volume is fixed, then doubling the absolute temperature will double the pressure.At 0° C, the absolute temperature is 273 K. Heat the gas to 273° C = 546 K.
Bubbles begin to form in a sample of liquid but the temperature did not change What must happened to cause the change?
The likely cause of bubbles forming in a liquid without a change in temperature is a decrease in pressure. When pressure decreases, gases dissolved in the liquid can come out of solution and form bubbles. This phenomenon is known as cavitation.
When scientists record the volume on a gas why do they also record the temperature and the pressure?
because the volume of the gas is dependent upon the temperature and pressure. This is also important in the identification of the molecular mass of an unknown gaseous element.
What happens to a fixed sample of gas when its temperature changes?
When the temperature of a fixed sample of gas changes, its particles will gain or lose kinetic energy, leading to a change in their speed and collisions. This results in a change in pressure and volume of the gas, according to the ideal gas law.
What would be the new pressure if a 400 mL gas sample at 380 mm Hg is expanded to 800 mL with no change of temperature?
According to Boyle's Law, if you double the volume of a gas at constant temperature, the pressure is halved. So, the pressure would decrease to 190 mm Hg when the gas sample is expanded to 800 mL.
What happens to the pressure of a sample gas if you double the volume and no change in the Kelvin temperature?
pV = nRT ← General Gas Lawrearranging to solve the pressure gives us:p = nRT/Vdoubling the volume gives: p = nRT/2VThis means that the pressure will be halved.
What happens to the partial pressure of oxygen in a sample of air when the temperature increases?
When the temperature of a sample of air increases, the partial pressure of oxygen also increases.
When a sample of gas is compressed from 6.0 L to 2.0 L at a constant temperature the pressure of the gas double?
Are you stating or asking ? If that's a statement, then it's an incorrect one. At constant temperature, the product of (pressure) x (volume) is constant. So, if the volume changed by a factor of 3, the pressure must also change by a factor of 3 ... the pressure must triple.
If the temperature is increased What happens to the partial pressure of oxygen in a sample of air?
If the temperature is increased, the partial pressure of oxygen in a sample of air will also increase. This is because as the temperature rises, the oxygen molecules in the air will have greater kinetic energy and will exert more pressure.
A gas sample is held at constant temperature. What happens to the pressure of the sample if the volume is doubled and the number of molecules is doubled?
If the volume is doubled and the number of molecules is doubled while the temperature is held constant, the pressure of the gas sample will remain the same. This is because both the volume and the number of molecules increased by the same factor, resulting in no net change in pressure according to the ideal gas law.
Which sample of water has the lowest vapor pressure?
The sample of water that has the lowest vapor pressure is the sample at a lower temperature. Vapor pressure decreases as temperature decreases because fewer molecules have enough energy to escape into the gas phase.
Imagine that bubbles begin to form a sample of liquid but the temperature did not change.what must have happened to cause this change?
The decrease in pressure caused the bubbles to form in the liquid sample without changing the temperature. This could occur, for example, if the liquid was moved to a region of lower pressure, releasing dissolved gases as bubbles.
What temperature change would cause a sample of an ideal gas to double in volume while the pressure was held constant?
If the volume is fixed, then doubling the absolute temperature will double the pressure.At 0° C, the absolute temperature is 273 K. Heat the gas to 273° C = 546 K.
Bubbles begin to form in a sample of liquid but the temperature did not change What must happened to cause the change?
The likely cause of bubbles forming in a liquid without a change in temperature is a decrease in pressure. When pressure decreases, gases dissolved in the liquid can come out of solution and form bubbles. This phenomenon is known as cavitation.
What sample is highly compressible at high pressure and expandable at high temperature?
liquid
