A 1.547 g sample of blue copper(II) sulfate pentahydrate, , is heated carefully to drive off the water. The white crystals of
1 answer:
Answer:
Explanation:
Hello,
By developing the following stoichiometric relationship, the required amount could be found as follows:
- Moles of :
- Grams of
- Moles of water:
Finally, one could see that the mass of the anhydrous compound is less than the pentahydrated compound since it is waterless.
Best regards.
You might be interested in
Answer:
14,448 J of heat would it take to completely vaporize 172 g of this liquid at its boiling point.
Explanation:
The heat Q that is necessary to provide for a mass m of a certain substance to change phase is equal to Q = m*L, where L is called the latent heat of the substance and depends on the type of phase change.
During the evaporation process, a substance goes from a liquid to a gaseous state and needs to absorb a certain amount of heat from its immediate surroundings, which results in its cooling. The heat absorbed is called the heat of vaporization.
So, it is called "heat of vaporization", the energy required to change 1 gram of substance from a liquid state to a gaseous state at the boiling point.
In this case, being:
- Q=?
- m= 172 g
- L= 84
and replacing in the expression Q = m*L you get:
Q=172 g*84
Q=14,448 J
<u><em>14,448 J of heat would it take to completely vaporize 172 g of this liquid at its boiling point.</em></u>