Question

A sample of pure NH4HS is placed in a sealed 2.0-L container and heated to 550 K at which the equilibrium constant is 3.5 x 10-3. Once the reaction reaches equilibrium, what mass of NH3 is present in the container

Answer 1

The mass of
`NH_(3)` in the container is 2.074 gram

Step-by-step explanation:

Given:

Volume of
`NH_(4) HS`
`V = 2` lit

Equilibrium constant
`k _(eq) = 3.5 * 10^(-3)`

The reaction in which
`NH_(3)` is produced

`NH_(4) HS` ⇄
`NH_(3) + H_(2)S`

Here equal moles of
`NH_(3)` and
`H_(2)S` is formed.

From the formula of equilibrium constant,

`k_(eq) = (NH_(3))(H_(2)S )`

`x^(2) = 3.5 * 10^(-3)`

`x = 0.061` M

Above value shows,

`NH_(3) = 0.061`
`(moles)/(L)`

So in 2 L no. moles of
`NH_(3)` =
`0.061 * 2 = 0.122` moles.

So mass of 0.122 mole of
`NH_(3)` is =
`0.122 * 17 = 2.074` g

Therefore, the mass of
`NH_(3)` in the container is 2.074 gram