A certain gas in expanded from `(1L, 10 atm)` to `(4L, 5 atm)` against a constant external pressure of `1atm`. If the initial temperature of gas is `300K` and heat capacity for the process is `50J^(@)C^(-1)`, the enthalpy change during the process is: (use: `1L-atm = 100J)`

Options

A. `Delta H = 15 KJ`
B. `Delta H= 15.7 KJ`
C. `Delta H=14.4 KJ`
D. `DeltaH=14.7 KJ`

Answer

B

Explanation

`Delta H=Delta E+Delta(PV)& Delta E=q+W=(50xx300-3xx100)J ["as" T_(f)=2xx300 K=600K]=14.7 KJ`
`Delta H=14700+10xx100=15700 J=15.7 KJ`.