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.
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
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