Question

Consider the dissociation of nitrosyl bromide: $2NOBr(g) \rightleftharpoons 2NO(g)+Br_{2}(g)$, The equilibrium constant, $K_{p}$, for the reaction is 0.0225 at 350°C. If a mixture contains 0.50 atm NOBr, 0.40 atm NO and 0.20 atm $Br_{2}$, will there be any net reaction? If so in which direction?

Answer 1

$2NOBr(g)\rightleftharpoons 2NO(g) + Br_2(g)$

A mixture contains 0.50 atm NOBr, 0.40atm NO and 0.20atm $Br_2$. To find if there will be any net reaction

Equilibrium is achieved at 350 degree,

$K_c= 0.0225 = K_F/K_R \\= (NOBR)^2/ (NO)^2(Br_2)$

⇒Since equilibrium constant is smaller, this means the reactants are way more than the products.

So the reaction will take place in opposite direction that is the reactant quantity shall be more than product.

Answer 2

i thought the written reaction is WRONG