Consider the equilibrium reaction and its equilibrium constant expression. Br 2 ( g ) + 2 NO ( g ) − ⇀ ↽ − 2 NOBr ( g ) K = [ NOBr ] 2 [ Br 2 ] [ NO ] 2 For the reaction 2 Br 2 ( g ) + 4 NO ( g ) − ⇀ ↽ − 4 NOBr ( g ) select the equilibrium constant expression.

Explanation:

Hello,

In this case, for the equilibrium condition, the equilibrium constant is defined via the law of mass action, which states that the division between the concentrations of the products over the concentration of the reactants at equilibrium equals the equilibrium constant, for the given reaction:

The suitable equilibrium constant turns out:

Or in terms of the initial equilibrium constant:

Since the second reaction is a doubled version of the first one.

Best regards.

answer: enthalpy

explanation:

for a exothermic reaction, the energy is released i.e. the energy of the products is lower than the energy of the reactants.

= enthaply

= energy of products

= energy of reactants

as , thus comes out to be negative. negative value of enthalpy shows that the reaction is exothermic.

i believe it is a.) released into

explanation: