Answer: 
, 
and 
are formed at the end of the reaction. They are named as tin (IV) oxide or stannic oxide, nitrogen dioxide and water respectively.
Explanation: Reaction of tin and nitric acid is given as:
Three products are formed at the end of the reaction which are:
- which is termed as stannic oxide or Tin (IV) oxide. This is a white colored solid.
- which is termed as nitrogen dioxide. These are brown colored fumes.
- which is termed as water.
At the starting tin was a silvery-white colored solid and after the reaction, it changed the color to milky-white. This change in color is due to the chemical reaction happening between tin and nitric acid.
Release of brown fumes are also an indication that a chemical reaction has taken place.
5.6 Al(OH)3
5.6 Al, 16.8 O, 16.8 H
16.8 mols of oxegyn in 5.6 mols of Al(OH)3
The Lewis dot diagram structure for hydrogen cyanide would be the following:
H - C --- N
--- = triple bond.
In this item, we are simply to find the ions that may bond and are able to form a formula unit. We are also instructed to give out their name. There are numerous possible combinations of ions to form a compound. Some answers are given in the list below.
1. Na⁺ , Cl⁻ , NaCl ---> sodium chloride (this is most commonly known as table salt)
2. C⁴⁺ , O²⁻ , CO₂ ---> carbon dioxide
3. Al³+ , Cl⁻ , AlCl₃ ----> aluminum chloride
4. Ca²⁺ , Cl⁻ , CaCl₂ ---> calcium chloride
5. Li⁺ , Br⁻ , LiBr ---> lithium bromide
6. Mg³⁺ , O²⁻ , Mg₂O₃ ----> magnesium oxide
7. K⁺ , I⁻ , KI ---> potassium iodide
8. H⁺ , Cl⁻ , HCl --> hydrogen chloride
9. H⁺ , Br⁻ , HBr ----> hydrogen bromide
10. Na⁺ , Br⁻ , NaBr ---> sodium bromide
The complete balanced chemical reactions are:
<span>HNO3 => CaCO3
+ 2HNO3 → Ca(NO3)2 + H2O + CO2(g)</span>
<span>H2SO4 => CaCO3
+ H2SO4 → CaSO4 + H2O + CO2(g) </span>
<span>So we see that 1 mole of CaCO3 is needed for 2 moles of HNO3 and similarly
to 1 mole of H2SO4.
</span>The number of moles can be calculated as the product of
volume and molarity, so:
moles H2SO4 = 1.7×10^−5 M * (15.5 x 10^9 L) = 263,500 mol
H2SO4
moles HNO3 = 8.9×10^−6 M * (15.5 x 10^9 L) = 137,950 mol
HNO3
So the total moles of CaCO3 required is:
moles CaCO3 = 263,500 mol * 1 + 137,950 mol * (1/2)
moles CaCO3 = 332,475 mol
The molar mass of CaCO3 is 100.086 g/mol, so the mass is:
mass CaCO3 = 332,475 mol * 100.086 g/mol
mass CaCO3 = 33,276,092.85 g = 33.3 x 10^3 kg
