Question

An initial mixture of nitrogen gas and hydrogen gas is reacted in a rigid container at a certain temperature by the reaction

3H2(g) +N2(g) <=> 2NH3(g)

At equilibrium the concentrations are [H2]=5.0 M, [N2]= 8.0M, [NH3]=3.0M

What were the concentrations of nitrogen gas and hydrogen gas that were reacted initially.

Answer 1

Answer: Concentrations of nitrogen gas and hydrogen gas that were reacted initially were 6.5 M and 0.5 respectively

Step-by-step explanation:

Equilibrium constant is the ratio of the concentration of products to the concentration of reactants each term raised to its stochiometric coefficients.

`3H_2(g)+N_2(g)\rightarrow 2NH_3(g)`

at t= 0 x y 0

tt t= eqm (x-3z) (y-z) 2z

2z = 3.0 M

z= 1.5 M

Initial concentration of
`H_2` =
`x-3* z = 5.0 M`

`x-3* 1.5 =5.0M`

`x=0.5M`

Initial concentration of
`N_2` =
`y-z =8.0M`

`y-1.5=8.0M`

`y=6.5M`

Thus concentrations of nitrogen gas and hydrogen gas that were reacted initially were 6.5 M and 0.5 respectively