A mixture of 0.2 mole of `N_(2)` and 0.6 mole of `H_(2)` react to give `NH_(3)` according to the equation, `N_(2)(g)+3H_(2)(g)iff2NH_(3)(g)` at constant temperature & pressure. 40 % mole of nitrogen react at equilibrium state. Then the ratio of the final volume to the initial volume of gases are

Options

A. `4 : 5`
B. `5 : 4`
C. `7 : 10`
D. `8 : 5`

Answer

A

Explanation

`N_(2)(g)+3H_(2)(g)iff2NH_(3)(g)`
mole `" 0.2 0.6 "`
Left mole `" 0.12 0.36 0.16"`
`therefore " "(V_(f))/(V_(i n))=(0.64)/(0.80) " "(because "T and P constant")`
`=0.8" or "(4 : 5)`