Question

a sample of carbon dioxide gas occupies a volume of 20 L at standard temperature and pressure (STP). what will be the volume of a sample of argon gas that has the same number of moles and but tripled the absolute temperature?​

Answer 1

Volume of Argon = 59.972 L

Further explanation

In general, the gas equation can be written  

$\large {\boxed {\bold {PV = nRT}}}$

where  

P = pressure, atm  

V = volume, liter  

n = number of moles  

R = gas constant = 0.08206 L.atm / mol K  

T = temperature, Kelvin  

At STP(0 C, 1 atm), 1 mol gas= 22.4 L

so for 20 L

$\tt \dfrac{20}{22.4}=0.893$

For Argon

P = 1 atm

T = 273 K x 3 =819 K (tripled)

n = 0.893 (the same number of moles)

R = 0.082 L/atm.mol K

$\tt V=\dfrac{nRT}{P}=\dfrac{0.893\times 0.082\times 819}{1}=59.972~L$