The local anesthetic ethyl chloride ( C2H5Cl, molar mass = 64.50
g
- according to the following balanced equation:
can be prepared by the reaction of ethylene ( C2H4, molar mass = 28.05
hydrogen chloride ( HC1, molar mass = 36.45
C2H4 + HCI -+ C2H5Cl
Assuming 14.00 g of ethylene and 24.00 g of hydrogen chloride are used, answer the following questions:
How many moles of hydrogen chloride are used? Be sure your answer has the correct number of significant figures.
moles of hydrogen chloride =
mol HC1
To find the moles of hydrogen chloride used, we first need to determine the limiting reactant in the reaction.
Calculate the moles of ethylene used:
moles = mass / molar mass
moles of C2H4 = 14.00 g / 28.05 g/mol = 0.499 moles
Calculate the moles of hydrogen chloride used:
moles of HCI = 24.00 g / 36.45 g/mol = 0.659 moles
Since the reaction utilizes 1 mole of ethylene and 1 mole of hydrogen chloride to produce 1 mole of ethyl chloride, the limiting reactant is ethylene, and 0.499 moles of hydrogen chloride are used in the reaction.
Therefore, the moles of hydrogen chloride used is 0.499 moles.