If 18.75 mol of helium gas is at 15.0°C and a gauge pressure of 0.400 atm,?
(a) calculate the
volume of the helium gas under these conditions. (b) Calculate the temperature if the gas is
compressed to precisely half the volume at a gauge pressure of 1.00 atm.
I really don't understand this question. Can someone please explain the steps. Thanks
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(a)
Step 1 convert 0.4atm to pascal (1atm = 101,000Pa); that's P.
Step 2 convert 15.0°C to kelvin (add 273); that's T
Step 3 put the numbers into the ideal gas equation PV = nRT
where n = 18.75mol
Rearrange the equation and find V (in m^3)
(b)
PV = nRT
iI V is halved and P is doubled, PxV is unchanged so nRT is unchanged.
Therefore there is no temperature change.