Answered

explain the effect of each of the following stresses on the position of the equilibrium so3(g) uv so2(g) 1 12 o2(g) the reaction as written is endothermic. (a) o2(g) is added to the equilibrium mixture without changing volume or temperature. (b) the mixture is compressed at constant temperature. (c) the equilibrium mixture is cooled. (d) an inert gas is pumped into the equilibrium mixture while the total gas pressure and the temperature are kept constant. (e) an inert gas is added to the equilibrium mixture with- out changing the volume.



Answer :

O₂ is a product. The addition of O₂ at constant volume and temperature will shift the equilibrium to the left is more reactants will be formed.

Endothermic reactions are the opposite of exothermic reactions. They soak up heat energy from their surroundings. which means the environment of endothermic reactions is less warm due to the response. Melting ice is an example of this type of response.

A. O₂ is a product. The addition of O₂ at constant volume and temperature will shift the equilibrium to the left is more reactants will be formed.

B. So₃(g) ------> So₂(g) 1 /2 o2(g)

n(g) reactant = 1

n(g) production = 1 + 0.5 = 1.5

n (g) > n (g) reactant

a number of product molecules increases.

The forward reaction is favored by low pressure as the high pressure will favor the reverse reaction.

An endothermic reaction occurs when the temperature of an isolated machine decreases whilst the environment of a non-isolated system gains warmness. Endothermic reactions result in an ordinary nice heat response

Learn more about endothermic here:-https://brainly.com/question/6506846

#SPJ4

Other Questions