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Stoichiometry Problems be SURE to BALANCE EACH EQUATION BEFORE SOLVING ANY PROBLEMS. SHOW YOUR SOLUTION. 3. Acetylene gas, C2H2 is used in welding, produces an extremely hot flame when it burns in pure oxygen according to the following reaction. c2h2 + o2 —> CO2 + H2O How many moles of water (h20) are produced when 27.20 grams of C2H2 burns completely?
Accepted Answer
1. Balance the Equation:
The balanced equation is:
2 C2H2 + 5 O2 → 4 CO2 + 2 H2O
2. Convert grams of C2H2 to moles:
Molar mass of C2H2 = (2
12.01 g/mol) + (2
1.01 g/mol) = 26.04 g/mol
Moles of C2H2 = 27.20 g / 26.04 g/mol = 1.04 mol
3. Use the mole ratio from the balanced equation to find moles of H2O:
From the balanced equation, 2 moles of C2H2 produce 2 moles of H2O.
Moles of H2O = (1.04 mol C2H2)
(2 mol H2O / 2 mol C2H2) = 1.04 mol H2O
Therefore, 1.04 moles of water (H2O) are produced when 27.20 grams of C2H2 burns completely.
The balanced equation is:
2 C2H2 + 5 O2 → 4 CO2 + 2 H2O
2. Convert grams of C2H2 to moles:
Molar mass of C2H2 = (2
12.01 g/mol) + (2
1.01 g/mol) = 26.04 g/mol
Moles of C2H2 = 27.20 g / 26.04 g/mol = 1.04 mol
3. Use the mole ratio from the balanced equation to find moles of H2O:
From the balanced equation, 2 moles of C2H2 produce 2 moles of H2O.
Moles of H2O = (1.04 mol C2H2)
(2 mol H2O / 2 mol C2H2) = 1.04 mol H2O
Therefore, 1.04 moles of water (H2O) are produced when 27.20 grams of C2H2 burns completely.
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