Asked by Dars
Given the following unbalanced equation
C4H10 (g) + O2 (g) → CO2 (g) + H2O (l)
What mass of water forms if 6.5 L of C4
H10 (g) measured at STP is allowed to react with 32.0 L of O2 (g)measured at 27°C and 1.68 atm pressure?
C4H10 (g) + O2 (g) → CO2 (g) + H2O (l)
What mass of water forms if 6.5 L of C4
H10 (g) measured at STP is allowed to react with 32.0 L of O2 (g)measured at 27°C and 1.68 atm pressure?
Answers
Answered by
DrBob222
2C4H10 + 13O2 ==> 8CO2 + 10H2O
mols C4H10 = 65L /22.4L = ?
mols O2 = use PV = nRT and solve for n.
Convert mols C4H1O to mols H2O using the coefficients in the balanced equation.
Do the same to convert mols O2 to mols H2O.
Probably the answers for mols H2O will not agree which means one of them is wrong. The correct answer in limiting reagent problems is ALWAYS the smaller value and the reagent producing that value is the limiting reagent.
The g H2O = mols H2O x molar mass H2O
mols C4H10 = 65L /22.4L = ?
mols O2 = use PV = nRT and solve for n.
Convert mols C4H1O to mols H2O using the coefficients in the balanced equation.
Do the same to convert mols O2 to mols H2O.
Probably the answers for mols H2O will not agree which means one of them is wrong. The correct answer in limiting reagent problems is ALWAYS the smaller value and the reagent producing that value is the limiting reagent.
The g H2O = mols H2O x molar mass H2O
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