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If pressure is held constant, volume and temperature are directly proportional. That is, as long as pressure is constant, if volume goes up so does temperature, if temperature goes down so does volume. This follows the model V1/T1=V2/T2, with V1 as initial volume, T1 as initial temperature, V2 as final volume, and T2 as final temperature.
When a gas is compressed, so volume is decreased, the pressure increases. P=1/V
Temperature is not directly tied to volume, its related to pressure. Increasing the temperature will increase the pressure--only if volume is held constant. That is were volume and temperature are related, through pressure. However, if you increase the volume it does not change the temperature.
when any gas is expanded, it's pressure would drop and the temperature would drop as well resulting with cold atmosphere.
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.
The resulting pressure will be 1.298 atm.
When air is compressed at the same temperate and volume space, pressure will increase in accordance with Boyle's Law which states: PV/T (initial) = PV/T (final) where P is pressure, V is volume and T is temperature.
If pressure is held constant, volume and temperature are directly proportional. That is, as long as pressure is constant, if volume goes up so does temperature, if temperature goes down so does volume. This follows the model V1/T1=V2/T2, with V1 as initial volume, T1 as initial temperature, V2 as final volume, and T2 as final temperature.
Assume temperature remains constant, then the pressure will rise in proportion to the decrease in volume, and vice versa.
A thermobarometer in a volumeter is used to measure both temperature and pressure, which are important factors in determining the volume of a substance. By taking into account temperature and pressure, the volumeter can accurately calculate the volume of the substance being measured.
When a gas is compressed, so volume is decreased, the pressure increases. P=1/V
Pressure, volume, temperature & the amount of gas.
Temperature is not directly tied to volume, its related to pressure. Increasing the temperature will increase the pressure--only if volume is held constant. That is were volume and temperature are related, through pressure. However, if you increase the volume it does not change the temperature.
Temperature is not directly tied to volume, its related to pressure. Increasing the temperature will increase the pressure--only if volume is held constant. That is were volume and temperature are related, through pressure. However, if you increase the volume it does not change the temperature.
Yes, a balloon shows that air can be compressed. The pressure in the balloon is higher than the pressure outside the balloon. The ideal gas law is PV = nRT where: P = pressure V = volume n = the number of moles of gas (the amount of gas) R = the ideal gas constant T = temperature So for the given volume of the balloon, and at a set temperature, if the pressure goes up, the amount of gas (the number of moles) must also go up. That means that the gas has been compressed.
A compressed fluid (also called a subcooled fluid) is a fluid under thermodynamic conditions that force it to be a steam. In a plot comparing absolute pressure and specific volume (commonly called a P-v diagram), of a real gas, a compressed fluid is to the left of the liquid-vapor phase boundary; that is, it will be to the left of the vapor dome.Some of the conditions that cause a fluid to be compressed are the following:§ A specific volume lesser than the specific volume of a saturated liquid§ A fluid temperature below the saturation temperature§ A pressure exceeding the saturation pressure§ An enthalpy smaller than the enthalpy of a saturated liquid
when any gas is expanded, it's pressure would drop and the temperature would drop as well resulting with cold atmosphere.