Two moles of n ideal gas are allowed to expand from a volume of `10dm^(3)` to `m^(3)` at 300 K against a pressure of 101.325 kPa. Calculate the work done

Options

A. `-20.16kJ`
B. `13.22kJ`
C. `-810.6J`
D. `-18.96kJ`

Answer

A

Explanation

Given, Number of moles (n)=2
Intial volume `(V_(1))=10dm^(3)=0.01m^(3)`
`(because1dm^(3)=(1)/(1000)m^(3))`
Final volume `(V_(2))=2m^(3)`
`P_("ext")=101.325kPa`
Temperature (T) = 300k
`because` Work done due to charge in volume against a constant pressure is given by
`W=-P_("ext")(V_(2)-V_(1))`
`:." "w=-101.325kPaxx(2-0.0.1)m^(3)`
`=-201.636kPam^(3)or-201.6kJ`
`(because1kJ=akPam^(3))`