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What is the mass, in mg, of carbon formed when 3.0 x 10^-3 mol of propene undergoes incomplete combustion? $$2C_3H_6 + 3O_2 ightarrow 6C + 6H_2O$$ - AQA - A-Level Chemistry - Question 11 - 2017 - Paper 3
Question 11
What is the mass, in mg, of carbon formed when 3.0 x 10^-3 mol of propene undergoes incomplete combustion? $$2C_3H_6 + 3O_2 ightarrow 6C + 6H_2O$$
Worked Solution & Example Answer:What is the mass, in mg, of carbon formed when 3.0 x 10^-3 mol of propene undergoes incomplete combustion? $$2C_3H_6 + 3O_2 ightarrow 6C + 6H_2O$$ - AQA - A-Level Chemistry - Question 11 - 2017 - Paper 3
Step 1
Calculate the moles of carbon formed
Answer
From the balanced equation, for every 2 moles of propene (), 6 moles of carbon (C) are produced. Therefore, the moles of carbon produced can be calculated as:
ext{Moles of carbon} = 6 imes rac{3.0 imes 10^{-3} ext{ mol } C_3H_6}{2} = 9.0 imes 10^{-3} ext{ mol C}.Step 2
Convert moles of carbon to mass
Answer
To find the mass of carbon formed in grams, we use the molar mass of carbon, which is approximately 12 g/mol.
ext{Mass of carbon} = 9.0 imes 10^{-3} ext{ mol} imes 12 rac{ ext{g}}{ ext{mol}} = 0.108 ext{ g}.To convert this to milligrams:
Thus, the answer corresponds to option C: 1.08 x 10^2 mg.