Answer:
B. Some of the absorbed energy is converted into potential energy, and some is converted into kinetic energy
Explanation:
Chemical energy is the kind of energy stored in the bonds formed by atoms and molecules in chemical compounds and elements. This energy is released during a chemical reaction and heat is often given out in the process. These kind of reactions where heat is given out as a by product are called exothermic reactions.
The major factor that determines how much chemical energy a substance has is the mass of that substance. Mass is defined as the amount of matter in a substance.
The higher the mass of a substance, the more concentrated that substance is and subsequently the greater the number of atoms and molecules.
Logically, the higher the number of atoms and molecules then the greater the number of bonds in that substance and subsequently the more the amount of chemical energy stored therein.
Answer:
A) NiBr₂ and AgNO₃
Explanation:
We can use the solubility rules to decide which reaction gives the precipitate.
The important ones for this problem are:
- Salts of Group I elements and of ammonia are soluble.
- Nitrates are soluble.
- Halides are soluble. Important exceptions the silver halides.
- Most sulfates are soluble.
- Most hydroxides are slightly soluble.
The possible products from each reaction are
A) Ni(NO₃)₂ and AgBr; B) NaBr and KI; C) KCl and Cr₂(SO₄)₃
D) KNO₃ and Ba(OH)₂; E) LiI and Cs₂CO₃.
A) Ni(NO₃)₂ and AgBr
Ni(NO₃)₂ — soluble (Rule 2)
AgBr — insoluble (an exception to Rule 3)
When aqueous solutions of NiBr₂ and AgNO₃ are mixed, a precipitate forms.
B) NaBr and KI
NaBr — soluble (Rule 1)
KI — soluble (Rule 1)
C) KCl and Cr₂(SO₄)₃
KCl — soluble (Rule 1)
Cr₂(SO₄)₃ — soluble (Rule 4)
D) KNO₃ and Ba(OH)₂
KNO₃ — soluble (Rule 1)
Ba(OH)₂ — soluble (Rule 5)
E) LiI and Cs₂CO₃
LiI — soluble (Rule 1)
Cs₂CO₃ — soluble (Rule 1)