Step 1:
Divide mass of each element with its M.mass in order to find out moles.
C = 63.2 g / 12 g/mol = Moles = 5.26 moles
H = 5.26 g / 1.008 g/mol = Moles = 5.21 moles
C = 41.6 g / 16 g/mol = Moles = 2.6 moles
Step 2:
Select moles of the element with least value and divide all moles of element by it,
C H O
5.26/2.6 : 5.21/2.6 : 2.6/2.6
2.02 : 2.00 : 1
Result:
Empirical Formula = C₂H₂O
Mass of SiC = 2 g
<h3>Further explanation</h3>
Given
Reaction
SiO₂(s) + 3C(s) → SiC(s) + 2CO(g)
3.00 g of SiO₂
4.50 g of C
Required
mass of SiC
Solution
mol SiO₂ (MW=60,08 g/mol) :
= 3 g : 60.08 g/mol
= 0.0499
mol C(Ar = 12 g/mol) :
= 4.5 g : 12 g/mol
= 0.375
mol : coefficient of reactants =
SiO₂ : 0.0499/1 = 0.0499
C : 0.375/3 = 0.125
SiO₂ as a limiting reactant(smaller ratio)
Mol SiC based on mol SiO₂ = 0.0499
Mass SiC :
= mol x MW
= 0.0499 x 40,11 g/mol
= 2 g
Answer:
2H3PO4 +3Ca(OH) 2 = Ca3 (PO4) 2 +6H20
Answer:
Aluminum sulfide or aluminium sulphide is a chemical compound with the formula Al2S3.
Explanation:
Answer: Strong acid vs weak acid
Strong acids and strong bases refer to species that completely dissociate to form ions in solution.
Explanation: By contrast, weak acids and bases ionize only partially, and the ionization reaction is reversible. Thus, weak acid and base solutions contain multiple charged and uncharged species in dynamic equilibrium.
