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. (a) `15 kJ`
B. (b) `15.7 kJ`
C. (c) `14.3 kJ`
D. (d) `14.7kJ`

Explanation

To find the enthalpy change (ΔH) during the expansion of the gas from (1L, 10 atm) to (4L, 5 atm) against a constant external pressure of 1 atm, we can follow these steps:

### Step 1: Calculate the number of moles (n) of the gas at state 1.
Using the ideal gas equation:
\[ PV = nRT \]
For state 1:
- \( P_1 = 10 \, \text{atm} \)
- \( V_1 = 1 \, \text{L} \)
...