A chemistry student is given 4.00 L of a clear aqueous solution at 22°C. He is told an unknown amount of a certain compound X is dissolved in the solution. The student allows the solution to cool to 22°C. The solution remains clear. He then evaporates all of the water under vacuum. A precipitate remains. The student washes, dries and weighs the precipitate. It weighs 0.56 kg. Required:
Using only the information above, can you calculate the solubility of X in water at 22°C. If you said yes, calculate it

No

Explanation:

It is given that :

Amount of the clear aqueous solution = 4 L

Temperature of the clear solution = 22°C

The solution remain clear even after an unknown amount of X compound is dissolved in the solution.

Then the water is evaporated under vacuum and the remaining precipitates weighs 0.56 kg.

Therefore, from the above data, we cannot calculate the solubility of the compound X that is added to the clear aqueous solution at 22°C.

The substance which gets dissolved is known as solute and the substance where the solute is dissolved is known as the solvent.

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.

the potential energy of the reactants is 200j.

from the energy diagram, the energy of the product formed is 350j; this means that, this reaction is an endothermic reaction, because it absorbs energy from its environment.