Butane (C_4 H_10) is used in lighten, and combusted with oxygen to produce carbo

Question

Butane (C_4 H_10) is used in lighten, and combusted with oxygen to produce carbon dioxide and water vapor. If 100 mL of is combusted, what volume of oxygen is required and what volumes of water vapor and carbon dioxide are produced? Potassium chlorate (40.44 grams) is decomposed to produce potassium chloride and oxygen gas at 740 mm-Hg and 525 degree C. What volume of oxygen is formed at the reaction conditions? Potassium chlorate (40.44 grams) is decomposed to produce potassium chloride and oxygen gas at 740 mm-Hg and 25 degree C. If the oxygen gas is collected over water at 25 degree C what is the volume of oxygen at standard conditions? If 0.5 mole of butane, C_4H_10, is reacted with 5 moles of oxygen to produce carbon dioxide and water, what are the partial pressure of all gases in the mixture at a total pressure of 2 atm? Answer #10: P_C4H10 = atm P_O2 = atm P_CO2 = atm P_H2O = atm

Explanation / Answer

7. moles of butane combusted = 100 ml x 0.0025 g/ml/58.1 = 0.0043 mols

moles of O2 needed = 0.0043 x 13 = 0.056 mols

Volume of O2 needed = 0.056 x 22.4 = 1.84 L O2

Volume of CO2 formed = 8 x 0.0043 x 22.4 = 0.77 L CO2

Volume of H2O formed = 10 x 0.0043 x 22.4 = 0.96 L H2P

8. 2KClO3 --> 2KCl + 3O2

moles of KClO3 = 40.44/122.55 = 0.33 mols

moles of O2 produced = 0.33 x 3/2 = 0.50 mols

Using,

V = nRT/P

Volume of O2 produced = 0.50 x 0.08205 x (525 + 273)/(740/760)

                                       = 33.623 L

9. When O2 is collected over water,

Pressure = (740 - 23.8)/760 = 0.942 atm

V = nRT/P

Volume of O2 produced = 0.50 x 0.08205 x (525 + 273)/0.942

                                       = 34.754 L

10. Total moles = 0.5 + 5 = 5.5 mols

Limiting reactant = butane

Partial pressure of butane (initial) = (0.5/5.5)2 = 0.2 atm

Partial pressure of O2 (initial) = (5/5.5)2 = 1.82 atm

After the reaction,

Partial pressure of butane (initial) = 0 atm

moles of CO2 = 2 mols

moles of H2O = 2.5 mols

moles of O2 = 1.75 mols

Total moles = 6.25 mols

Partial pressure of O2 (final) = (1.75/6.25)2 = 0.56 atm

Partial pressure of CO2 = (2/6.25)2 = 0.64 atm

Partial pressure of H2O = (2.5/6.25)2 = 0.8 atm

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