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a_sh-v [17]
3 years ago
13

A 5.00-l tank contains helium gas at 1.50 atm. what is the pressure of the gas in torr if volume is doubled

Chemistry
1 answer:
vazorg [7]3 years ago
5 0
<span>570 torr. The ideal gas law is PV = nRT where P = pressure V = volume n = number of moles of gas particles R = Ideal gas constant T = absolute temperature Since the value n, R, and T remain constant for this problem, that indicates that if the volume is doubled, the pressure will be halved. So the new pressure will be 1.50 atm / 2 = 0.750 atm. Now we just need to convert that from atm to torr. 1 atm is equal to 760 torr, so 0.750 atm * 760 torr/atm = 570 torr.</span>
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