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