What temperature would 3.54 moles of xenon gas need to reach to exert a pressure of 1.57 atm at a volume of 34.6 l

186.9Kelvin

Explanation:

The ideal gas law equation is PV = n R T

where

P is the pressure of the gas

V is the volume it occupies

n is the number of moles of gas present in the sample

R is the universal gas constant, equal to 0.0821 atm L / mol K

T is the absolute temperature of the gas

Ensure units of the volume, pressure, and temperature of the gas correspond to R (the universal gas constant, equal to 0.0821 atm L / mol K)

n = 3.54moles

P = 1.57

V = 34.6

T=?

PV = n R T

PV/nR = T

1.57 x 34.6/3.54 x 0.0821

54.322/0.290634 = 186.908620464 = T

186.9Kelvin (approximately to 1 decimal place)