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If a gas with a volume of 525ml at a temp of -25Celsius is heated to 175Celsius what us the new volume of the gas pressure and the number of the moles are held constant?
Wiki User
∙ 12y ago
Assuming the gas follows the ideal gas law (which at these temperatures and pressures should be a good assumption),
T2/T1 = P2V2/P1V1
so
T2 (final temperature) = T1 x P2V2/P1V1
Temperature has to given in absolute temperature for this to work, so we first convert T1 25°C = 278.15 K.
T2 = (278.15 K)(47.3 kPa)(7.0 L)/(95.3 kPa)/(2 L) = ~386.55 K = ~113.40 °C
If it seems strange to you that the temperature went UP when the gas expanded, consider this...
If the temperature remained constant, then as the pressure dropped to 47.3 kPa, the volume would only increase to about 5 L. To make the volume increase to 7 L at that pressure you would have to heat the gas up get it to expand.
Wiki User
∙ 8y ago
Wiki User
∙ 13y agoYou did not give enough information to solve this question.
For basic question of pressure and volume you use the formula PV=nRT
P-pressure (in atm)
V-volume (in L)
n-number of mols
R-.08206 (Avagadro's number)
T-temperature (in K)
You need to know the number of mols of gas and temperature in order to figure this out.
Wiki User
∙ 8y agop1v1=p2v2
(710)(625)=(760)(v)
443750=760v
443750/760=583.88
583.88
Wiki User
∙ 12y ago948 ml
Wiki User
∙ 12y ago1556mmHg
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