1 g of water at `100^@C` is completely converted into steam at `100^@C`. 1 g of steam occupies a volume of 1650 cc . (Neglect the volume of 1 g of water at `100^@C`). At the pressure of `10^(5)N//m^(2)`, latent heat of steam is `540cals//g` (1 Calorie= 4.2 Joules).The increase in the internal energy in Joules is

Options

A. 2310
B. 2203
C. 1650
D. 2150

Explanation

Heat required to convert 1 g of water at `100^(@)C` completely into steam at ` 100^(@)C`
dQ = mL
`1 xx 540` calorie
`= 540 xx 42 = 2268` j
Work done in expanding volume
`dW = pdV = 10^(5) (V_(2) - V_(1))`
`= 10^(5) (1650 - 1000) xx 10^(6)`
`=650 xx 10^(-1) = 65`
Increase in internal energy
dU = dQ - dW = 2268 - 65 = 2203 J