If 21.4 g of carbon dioxide is produced in the reaction of ethyne with oxygen to form carbon dioxide and water, how many grams of water are produced in this reaction?
a) 8.76 g
b) 4.38 g
c) 17.5 g
d) 2.92 g
e) None of these
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The chemical equation for the reaction of ethyne (C2H2) with oxygen (O2) to form carbon dioxide (CO2) and water (H2O) is:
C2H2 + 5O2 → 2CO2 + 2H2O
According to the balanced equation, for every 2 moles of carbon dioxide produced, 2 moles of water are produced.
To find the grams of water produced, we can use the molar mass of water, which is 18.015 g/mol.
First, we calculate the number of moles of carbon dioxide produced:
mass of CO2 = 21.4 g CO2
molar mass of CO2 = 44.01 g/mol (C: 12.01 g/mol, O: 16.00 g/mol)
moles of CO2 = mass of CO2 / molar mass of CO2 = 21.4 g CO2 / 44.01 g/mol = 0.486 mol CO2
Since the coefficient ratio between CO2 and H2O is 2:2, the same amount of moles is produced for water.
Now, we calculate the mass of water produced:
moles of H2O = 0.486 mol H2O
molar mass of H2O = 18.015 g/mol
mass of H2O = moles of H2O × molar mass of H2O = 0.486 mol H2O × 18.015 g/mol = 8.757 g H2O
So, the answer is approximately 8.76 g of water (option a).
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