The combustion of any hydrocarbon yields water and carbon dioxide. We will now construct a balanced equation:
C₃H₈ + 5O₂ → 3CO₂ + 4H₂O
Each mole of propane requires 5 moles of oxygen.
Answer:
4.78 %.
Explanation:
<em>mass percent is the ratio of the mass of the solute to the mass of the solution multiplied by 100.</em>
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<em>mass % = (mass of solute/mass of solution) x 100.</em>
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mass of MgSO₄ = 50.0 g,
mass of water = d.V = (0.997 g/mL)(1000.0 mL) = 997.0 g.
mass of the solution = mass of water + mass of MgSO₄ = 997.0 g + 50.0 g = 1047.0 g.
<em>∴ mass % = (mass of solute/mass of solution) x 100</em> = (50.0 g/1047.0 g) x 100 = <em>4.776 % ≅ 4.78 %.</em>
The formula to find yield is
(Actual Yield)/(Theorectical Yield) x100
Just do the math.
85.22% x 113 = 96.2986
Convert it to 3 significant figures
Ans: 96.3g
Answer:
hydroperoxyethane
Explanation:
tomsFor the Lewis structure we have to remember that all the atoms must have <u>8 electrons</u> (except for hydrogen). In this structure, we have three types of atoms, Carbon, Hydrogen and Oxygen. So, we have to remember the <u>valence electrons</u> for each atom:
-) Carbon : 4 electrons
-) Hydrogen: 1 electron
-) Oxygen: 6 electrons
We can start with the "
" part. We can put 3 hydrogen bond arroun the carbon. We can use this same logic with "
". Finally for oxygens, we can put it one bond with and a bond between oxygens with a final bond with hydrogen to obtain <u>hydroperoxyethane</u>.
See figure 1 for further explanations.
