A 3.00 L cylinder at 25 degrees Celsius contains a mixture of 3 gases: He, N2, and Ar at partial pressures of 115, 285, and 325 torr, respectively. If all the He is removed from the mixture and the temperature does not change, what will be the partial pressure, in torr, of the N2

Explanation:

Given that

Volume of cylinder = 3 L

Temperature= 25 degrees

Partial pressure of the gases

By using Dalton's law , the total pressure of the non reacting gas is the sum of the partial pressure of all gases.

When all the He gas will removed then partial pressure of He will be zero.

Partial pressure of N₂

i believe it is a.) released into

explanation:

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.