To determine the moles of chloroform formed, we first need to identify the limiting reactant.
1. Calculate the moles of methane used:
moles of CH4 = mass / molar mass
moles of CH4 = 10.50g / 16.04 g/mol
moles of CH4 ≈ 0.654 mol
2. Calculate the moles of chlorine used:
moles of Cl2 = mass / molar mass
moles of Cl2 = 20.50g / (35.45 g/mol + 35.45 g/mol)
moles of Cl2 ≈ 0.289 mol
3. Determine the limiting reactant:
Since the balanced equation shows that 1 mole of methane reacts with 3 moles of chlorine, we need to determine how many moles of chlorine would react with the moles of methane determined.
moles of Cl2 needed = (moles of CH4) x 3
moles of Cl2 needed ≈ 0.654 mol x 3 ≈ 1.963 mol
Since we only have 0.289 mol of Cl2, it is the limiting reactant.
4. Calculate the moles of chloroform formed using the limiting reactant:
moles of CHCl3 = moles of limiting reactant
moles of CHCl3 ≈ 0.289 mol
Therefore, approximately 0.289 moles of chloroform are formed.
The anesthetic chloroform (CHCI3, molar mass=119.36 g/mol) can be prepared by the reaction of methane CH4 molar mass= 16.04 g/mol with chlorine according to the following balanced equation: CH4+3CI2 CHCI3+3HCI
Assuming 10.50g of methane and 20.50g of chlorine are used, answer the following questions:
How many moles of chloroform are formed? Be sure your answer has the correct number of significant figures.
moles of chloroform
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