Which of the following actions would cause the volume of the chamber below to increase to 36.0 L?

Option C. Triple the number of moles

Explanation:

From the ideal gas equation:

PV = nRT

Where:

P is the pressure

V is the volume

n is the number of mole

R is the gas constant

T is the absolute temperature.

Making V the subject of the above equation, we have:

PV = nRT

Divide both side by P

V = nRT / P

Thus, we can say that the volume (V) is directly proportional to both the number of mole (n) and absolute temperature (T) and inversely proportional to the pressure (P). This implies that and increase in either the number of mole, the absolute temperature and a decrease in the presence will cause the volume to increase.

Thus, the correct option is option C triple the number of moles. This can further be seen as illustrated below:

Initial volume (V1) = 12 L

Initial mole (n1) = 0.5 mole

Final mole (n2) = triple the initial mole = 3 × 0.5 = 1.5 mole

Final volume (V2) =?

From:

V = nRT / P, keeping T and P constant, we have:

V1/n1 = V2/n2

12/0.5 = V2/1.5

24 = V2/1.5

Cross multiply

V2 = 24 × 1.5

V2 = 36 L.

Thus Option C gives the correct answer to the question.

dynamic equilibrium is the answer.

a. energy is absorbed in the reaction.

if in a given reaction the energy of products is greater than the energy of reactants it means that reaction is endothermic and during the reaction, the energy is absorbed by reactants. in an endothermic reaction, the products have more stored chemical energy than the reactants. and in this reaction the reactants are more stable than products before the compounds with less energy are always more stable.