Question

Two moles of carbon monoxide (CO) start at a pressure of 1.5 atm and a volume of 29 liters . The gas is then compressed adiabatically to 13 this volume. Assume that the gas may be treated as ideal.

(a) What is the change in the internal energy of the gas? Does the internal energy increase or decrease?
(b) Does the temperature of the gas increase or decrease during this process? Explain.

Answer 1

Step-by-step explanation:

Initial temperature of gas = pv / nR

= 1.5 x 29 / 2 x .082

= 265K

We can calculate the final temperature of gas as follows

T₂ = T₁
`((V_1)/(V_2))^(1.4-1)`

= 265 x 3°⁴

= 411K

Rise in temp = 411 - 265

= 146

increase in internal energy

=n
`C_VdT`

= 2x 5/2 R X 146

= 6059 J

Since there is rise in temperature , there will be rise in internal energy.