If 42.5 mol of an ideal gas is at 8.77 atm and 439 K, what is the volume of the gas?

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Answer 1 · 2018-02-28T08:53:08

Well, is not #PV=nRT#?

And so ...#V=(nRT)/P#

#=(42.5*molxx0.0821*(L*atm)/(K*mol)xx439*K)/(8.77*atm)#

#=??*L#...I make this approx. #175*L#...

Answer 2 · 2018-02-28T08:53:41

The volume of the gas is #175# liters.

To solve this problem, we need to use the ideal gas law:

#PV=nRT#

#P# is pressure in atmospheres, #V# is volume in liters, #n# is moles, #R# is the universal gas constant, and #T# is the temperature in Kelvins.

Plug the known values into the equation and solve for the volume.

#(8.77)(V)=(42.5)(0.08206)(439)#

#V=((42.5)(0.08206)(439))/(8.77)=175# liters