P V = k T, so at constant temperature, PV is constant Initial PV = (102.5 x 3.67) = 376.175 ====> At constant temp, V = (376.175 / P) Final P = 100.9. Final V = (376.175 / 100.9) = 3.7282 L (rounded)
PV = RT is the ideal gas law P-pressure V-volume R-gas constant T-temperature then the equation becomes PV = constant therefore P = 1/V pressure becomes inversely proportional to the volume. hence as the volume increases the pressure decreases.
You can calculate pressure and temperature for a constant volume process using the combined gas law.
In dual combustion cycle heat is added at constant volume which increases the efficiency of cycle, whereas heat addition at constant pressure limits the maximum pressure of the cycle.
According to a calculator I used The New Temperature is -178.2 This is using PV = NRT and with only 1 mole of gas calculate the volume first with the stuff you gave and then calculate the new value using that volume Just like magic you get -178.2 Celsius Ps i did use 2870 and 8440 which are the above pressures but not in standard form.
compressor work on two principles 1)reduce volume of a constant amount of gas 2)adding more gas in a constant amount of volume positive displacement compressor works on first principle it reduces the volume of gas by applying force on it but gas amount is constant in every stroke or rotation thus increasing the pressure. centrifugal compressor work on second principle it adds more amount of gas in a given constant volume thus the pressure increase.
A sample of gas occupies 1.55L at STP. What will the volume be if the pressure is increased to 50 atm while the temperature remains constant?
Charles's law states that at constant pressure, the volume of a given mass of an ideal gas increases or decreases by the same factor as its absolute temperature. For fixed mass of an Ideal Gas at constant pressure the volume it occupies is directly proportional to its absolute temperature. So, if you double the absolute temperature of a gas while holding its pressure constant, the volume has to double. There is no such thing as an Ideal Gas. So, doubling the temperature of a real gas will not exactly double its volume. However, the general principle hold true. If you increase the temperature of any gas at constant pressure the volume it occupies will increase.
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At constant temperature p.V=constant, so pressure INcreases when decreasing the volume.
Temperature increases as pressure increases.
Increasing the temperature of a gas will increase it's pressure ONLY if the volume is held constant.
The product of pressure and volume. Does PV = nRT look familiar? (:
If the volume is constant, the density does not change with temperature. With increasing temperature there is still the same number of molecules confined to the same volume of space, so no difference in density.
It can but, not necessarily so. At a constant volume the temperature and pressure rise in direct proportion. At a constant temperature the volume is inversely proportionate to the pressure. At a constant pressure the volume is directly proportionate to the temperature.
When the temperature of a gas is increased at a constant pressure, its volume increases. When the temperature of a gas is devreased at constnt pressure, its volume decreases.
as the pressure decreases the volume of gas increases at constant temperature
Volume & pressure are inversely proportionate, if temperature stays constant volume would decrease at a factor proporionate to the increase in pressure.