A container holds 1.1 g of argon at a pressure of 8.0 atm. you may want to review (pages 382 - 383). how much will the temperature increase if this amount of heat energy is transferred to the gas at constant pressure? express your answer using two significant figures.

When heat energy at a constant pressure = the change of enthalpy

ΔH = Q

and when the internal energy of an ideal gas formula is:

ΔH = n. Cp.ΔT

and when Cp = (5/2) R at a constant pressure of a monatomic ideal gas

∴Q = n. (5/2). R.ΔT

∴ ΔT = Q / [n. (5/2). R]

when Q is the heat required = 43.08 J (given)

and n is no. of moles = mass / molar mass

= 1.1 g / 39.948 g/mol

= 0.0275 moles

and R is gas constant = 8.314472J/mol K

by substitution:

ΔT = 43.08 J / (0.0275moles * (5/2) * 8.314472 J/mol K

= 76.76 K