Dinitrogen tetraoxide and nitrogen dioxide are two gases that exist in equilibrium at a range of temperatures. no2 is a reddish brown gas while n2o4 is colorless. at high temperature the red color is strong. at low temperature the gas has less color. if we represent the equilibrium as: 2 no2(g) n2o4(g)

if we represent the equilibrium as: 2 no2(g) doublearrow. gifn2o4(g)
we can conclude that:

this reaction is:

a. exothermic
b. endothermic
c. neutral
d. more information is needed to answer this question.

A. Exothermic

Explanation:

Let's consider the following reaction at equilibrium.

    2 NO₂(g)       ⇄      N₂O₄(g)

reddish brown         colorless

In order to assess the effect of temperature on the equilibrium, we need to consider Le chatelier's principle: If a system at equilibrium suffers a perturbation, it will shift its equilibrium position to counteract such perturbation.

Let's suppose the reaction is exothermic.

Since it coincides with the experimental results, we can conclude that the reaction is exothermic.

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