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A gas has a pressure of 1.26 ATM and occupies a volume of 7.40 L If the gas is compressed to a volume of 2.93 L what will its pressure be assuming constant temperature?
Wiki User
∙ 12y ago
Verified answer
P1= 1.26 ATM
V1= 7.60 L
V2= 2.93 L
P2= ?
P1V1= P2V2
.
. . P2= 1.26 x 7.60 /2.93
= 3.27 ATM
Wiki User
∙ 12y ago
Wiki User
∙ 12y agoPV = nRT
Therefore, in state 1 P = 1 ATM, V = 21 L, and T = 298 K.
R is the universal gas constant. Since the number of moles, n, does not change you can equate state 1 and 2 and solve for the temperature of state 2.
PV/T of state 1 = 1 ATM * 21 L / 298
PV/T of state 2 = 1 ATM * 56.1 L / T2
i.e. 21/298 = 56.1/T2 and solve for T2
Wiki User
∙ 14y agoWhat level are you at? Assuming gas is ideal gas then use boyle's law. P over V of original condition equals P over V of new condition. This assumes same no. of mole of gas and temperature.
Anonymous
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Anonymous
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