Question #a9607

1 Answer
Jul 7, 2017

Answer:

#4.0 xx 10^2# #"K"#

Explanation:

We can use the ideal gas equation to solve this problem:

#PV = nRT#

where

  • #P# is the pressure exerted by the gas, in #"atm"#

  • #V# is the volume occupied by the gas, in #"L"#

  • #n# is the number of moles of gas present

  • #R# is the universal gas constant, equal to #0.082057("L"•"atm")/("mol"•"K")#

  • #T# is the absolute temperature of the gas, in #"K"#

Since all our units are appropriate, let's plug things in and solve for #T#:

#T = (PV)/(nR)#

#= ((1.5cancel("atm"))(12.9cancel("L")))/((0.59cancel("mol"))(0.082057(cancel("L")•cancel("atm"))/(cancel("mol")•"K"))) = color(red)(4.0xx10^2# #color(red)("K"#

rounded to two significant figures.