First convert each mass to moles by dividing by the molar mass.
0.347g Oxygen = 0.022 moles
0.260g Carbon = 0.022 moles
1.537g Chlorine = 0.043 moles
Divide each by smallest mole vale (0.022)
Oxygen = 0.022/0.022 = 1
Carbon = 0.022/0.022 = 1
Chlorine = 0.043/0.022 = 2
Therefore the empirical formula is COCl2
Answer:
cornell noted
Explanation:
used in middle school and can be helpful for subjects like ela history and science
Ksp=3.45×10⁻¹¹
CaF₂(s) ⇄ Ca²⁺(aq) + 2F⁻(aq)
Ksp=[Ca²⁺][F⁻]²
[Ca²⁺]=C(CaF₂)
[F⁻]=2C(CaF₂)
Ksp=4{C(CaF₂)}³
C(CaF₂)=∛(Ksp/4)
C(CaF₂)=∛(3.45×10⁻¹¹/4)=2.05×10⁻⁴ mol/L
2.05×10⁻⁴ M
Answer:
CuSO4(aq) + 4NH3(aq) + nH2O→ [Cu(NH3)4H2On]S04(aq)
Explanation:
When the concentrated ammonia is added into the copper ions solution, a blue solid is formed. This blue solid is gelatinous.it consist of Cu(OH)2 in insoluble form. As more ammonia is added precipitate start to dissolve and [Cu(NH3)4]∧+2 is produce.
Net Ionic equation:
Cu∧+2 +4NH3 → [Cu(NH3)4]∧+2
S04∧-2 are spectator ions.
Properties and uses of Tetraaminecopper(ll) sulfate:
1. It is solid compound.
2. Its color is dark blue.
3. It has ammonia like odor.
4. It is used to make the copper compounds and also used in the printing of fabric.
5. It is also used as pesticide.
Answer : The value of 
for the reaction is, -521.6 kJ
Explanation :
According to Hess’s law of constant heat summation, the heat absorbed or evolved in a given chemical equation is the same whether the process occurs in one step or several steps.
According to this law, the chemical equation can be treated as ordinary algebraic expression and can be added or subtracted to yield the required equation. That means the enthalpy change of the overall reaction is the sum of the enthalpy changes of the intermediate reactions.
The given main reaction is,
The intermediate balanced chemical reaction will be,
(1) 
(2) 
Now we are multiplying reaction 1 by 2 and reversing reaction 2 and then adding all the equations, we get :
(1) 
(2) 
The expression for enthalpy of change will be,
Thus, the value of for the reaction is, -521.6 kJ
