Please show all your work, thanks!
Solution :-
Using the volume and the density lets calculate the mass of the 1-heptene
Mass = volume * density
= 10 ml * 0.67 g per ml = 6.7 g 1-heptene
Now lets calculate the moles of the both reactants
Moles = mass / molar mass
Moles of 1-heptene = 6.7 g / 98.186 g per mol = 0.0682 mol
Moles of HBr = 5.1 g / 80.91 g per mol = 0.063 mol HBr
Mole ratio of the both reactants with product is 1 : 1 and moles of the HBr are less therefore HBr is the limiting reactant
So moles of the product that can be formed are same as moles of HBr
So moles of the 2-bromoheptane = 0.063 moles
Now lets convert moles of the product to its mass
Mass = moles * molar mass
Mass of 2-bromoheptane = 0.063 mol * 179 g per mol
= 11.3 g
Therefore theoretical yield = 11.3 g
Now lets calculate the percent yield
Percent yield = (actual yield / thereotical yield )* 100 %
= (8.7 g / 11.3 g)*100%
= 76.99 %
Therefore the percent yield = 76.99 %
Please show all your work, thanks! When 10 mL of 1-heptene was reacted with 5.1 grams...
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