balance 1-butanol + oxygen=carbon dioxide+water how many grams of carbon dioxide and water are produced when 130.6 grams of 1-butanol is completly burned?
YOu have to do a balanced chemical equation. Do that. Then examine the mole ratios
To balance the given chemical equation:
1-butanol + oxygen -> carbon dioxide + water
1. Write down the unbalanced equation:
C4H10O + O2 -> CO2 + H2O
2. Balance the carbon atoms first:
C4H10O + O2 -> 4 CO2 + H2O
3. Balance the hydrogen atoms next:
C4H10O + O2 -> 4 CO2 + 5 H2O
4. Finally, balance the oxygen atoms:
C4H10O + 6.5 O2 -> 4 CO2 + 5 H2O
Now that the equation is balanced, we can calculate the mass of carbon dioxide (CO2) and water (H2O) produced when 130.6 grams of 1-butanol is completely burned.
Molar mass of 1-butanol (C4H10O) = 74.12 g/mol
Molar mass of carbon dioxide (CO2) = 44.01 g/mol
Molar mass of water (H2O) = 18.02 g/mol
1. Calculate the number of moles of 1-butanol:
Moles of C4H10O = Mass of C4H10O / Molar mass of C4H10O
Moles of C4H10O = 130.6 g / 74.12 g/mol ≈ 1.764 mol
2. Determine the moles of CO2 produced:
According to the balanced equation, the ratio of C4H10O to CO2 is 1:4.
Moles of CO2 = Moles of C4H10O x (4 moles of CO2 / 1 mol of C4H10O)
Moles of CO2 = 1.764 mol x (4 mol CO2 / 1 mol C4H10O) = 7.056 mol
3. Calculate the mass of carbon dioxide:
Mass of CO2 = Moles of CO2 x Molar mass of CO2
Mass of CO2 = 7.056 mol x 44.01 g/mol ≈ 310.55 g
4. Determine the moles of H2O produced:
According to the balanced equation, the ratio of C4H10O to H2O is 1:5.
Moles of H2O = Moles of C4H10O x (5 moles of H2O / 1 mol of C4H10O)
Moles of H2O = 1.764 mol x (5 mol H2O / 1 mol C4H10O) = 8.82 mol
5. Calculate the mass of water:
Mass of H2O = Moles of H2O x Molar mass of H2O
Mass of H2O = 8.82 mol x 18.02 g/mol ≈ 158.86 g
Therefore, when 130.6 grams of 1-butanol is completely burned, approximately 310.55 grams of carbon dioxide and 158.86 grams of water are produced.