C₄H₉OH + HBr = C₄H₉Br + H2O
Δmole of alcohol gives 1 mole of bromobutanol
HBr is in excess, so the yield of the product is limited by the alcohol
Wt. of 1 butanol = 18
Molar mass of the butanol = 74.12 g/mole
Moles of the alcohol = 1/74.12 = 0.01349 moles
So, moles of bromobutane = 0.01349 moles
Molar mass of C₄H₉Br = 137.018 g/moles
So, theoretical mass of bromobutane is = 0.01349 × 137.0.18
= 1.85 g
Answer:
B
Explanation:
Homogeneous= all particles are dissolved thoroughly
Solute= 1 gram of salt
Solvent= 500 mL water
They use it because it's standerize and evidence vase
Answer:Molarity
Explanation:M stand for molarity
Answer:
No, a mole of oxygen is about 16 grams
Explanation:
