In the reaction between #HNO_2# and #HCN#: #HNO_2(aq) + CN^(-)(aq) rightleftharpoons HCN(aq) + NO_2^(-)(aq)#, K = #1 x 10^6#. What are the predominate species after the reaction reaches equilibrium?

1 Answer
May 14, 2017

Answer:

Which side do you think is favoured by the equilibrium?

Explanation:

For #A+BrightleftharpoonsC+D#, we define #K_"eq"=([C][D])/([A][B])#

If #K_"eq"# is LARGE, which it most certainly is, then it follows that the quotient #([C][D])/([A][B])# is also large, and this means that the concentrations of #C# and #D#, the PRODUCTS are favoured at equilibrium.

Given that the following reaction has reached equilibrium:

#HNO_2(aq) + N-=C^(-)rightleftharpoonsNO_2^(-) + HC-=N(aq)#,

.............it follows that there are large concentrations of #HC-=N# and #"nitrite anion"#.

Why would you NOT want to be downwind of this reaction?