Acontainer 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.

The change in temperature of the gas is 60.02°C

Data;

Mass = 1.1gPressure = 8.0 atmThe Number of Moles

The numbers of moles present is needed to calculate the Cv value of the gas.

The Cv value of the gas is

The energy of the gas will be

The energy on the gas is 33.67J

However,

But Cp is given as

Let's substitute the values and solve

The change in temperature of the gas is 60.02°C

Learn more on Cv, Cp value of a gas here;

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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 

Hi. where is the graph?

100%sorry if i’m wronghope this good luck: )