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

Question

2019 views around the world

You can reuse this answer
Creative Commons License

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