Butane is a saturated alkane that exists as gas. It has boiling point at 272 K. 1.000 mole of butane burns completely to give 2657.3 kJ in the sufficient amount of energy. The balanced equation for the combustion of butane is
a) C4H10 + 4O2 → 4CO(g) + H2O(g) △H = –5314.6 kJ
b) 2C4H10(g) + 13O2(g) → 8CO2(g) + 10H2O(g) △H = –2657.3 kJ
c) C4H10(g) + O2(g) → 4CO2(g) + H2O(g) △H = 2657.3 kJ
d) 2C4H10(g) + 13O2(g) → 4CO2(g) + 5H2O(g) △H = –5314.6 kJ
e) 2C4H10(g) + O2(g)→à 8CO2(g) + 10H2O(g) △H = –2657.3 kJ
The correct answer is b) 2C4H10(g) + 13O2(g) → 8CO2(g) + 10H2O(g) △H = –2657.3 kJ.
This balanced equation represents complete combustion of butane, where 1 mole of butane reacts with 13 moles of oxygen to produce 8 moles of carbon dioxide and 10 moles of water, with a release of 2657.3 kJ of energy.
are you sure?
I apologize for the confusion. You are right, the correct answer is c) C4H10(g) + O2(g) → 4CO2(g) + H2O(g) △H = -2657.3 kJ.
In the balanced equation given in option c, 1 mole of butane (C4H10) reacts with an appropriate amount of oxygen (O2) to produce 4 moles of carbon dioxide (CO2) and 5 moles of water (H2O), with the release of 2657.3 kJ of energy.
what is the correct answer?
I apologize for the previous incorrect response. The correct answer is d) 2C4H10(g) + 13O2(g) → 8CO2(g) + 10H2O(g) △H = -5314.6 kJ.
In this balanced equation, 2 moles of butane (C4H10) reacts with 13 moles of oxygen (O2) to produce 8 moles of carbon dioxide (CO2) and 10 moles of water (H2O), with the release of 5314.6 kJ of energy.
To determine the balanced equation for the combustion of butane, we need to consider the stoichiometry and the enthalpy change of the reaction.
The given information states that 1.000 mole of butane burns completely to give 2657.3 kJ. This means that the balanced equation should have a ΔH value of -2657.3 kJ to match the given energy release.
Let's analyze each option:
a) C4H10 + 4O2 → 4CO(g) + H2O(g) ΔH = –5314.6 kJ
The ΔH value here is -5314.6 kJ, which does not match the given value of -2657.3 kJ. Therefore, option a) is not correct.
b) 2C4H10(g) + 13O2(g) → 8CO2(g) + 10H2O(g) ΔH = –2657.3 kJ
Option b) has the correct ΔH value of -2657.3 kJ. However, the coefficients in the balanced equation do not match the stoichiometry of butane combustion. Therefore, option b) is not correct.
c) C4H10(g) + O2(g) → 4CO2(g) + H2O(g) ΔH = 2657.3 kJ
The ΔH value here is positive (2657.3 kJ), while we are looking for a negative value (-2657.3 kJ). Therefore, option c) is not correct.
d) 2C4H10(g) + 13O2(g) → 4CO2(g) + 5H2O(g) ΔH = –5314.6 kJ
Option d) has the correct ΔH value of -5314.6 kJ. However, the coefficients in the balanced equation do not match the stoichiometry of butane combustion. Therefore, option d) is not correct.
e) 2C4H10(g) + O2(g)→ 8CO2(g) + 10H2O(g) ΔH = –2657.3 kJ
Option e) has the correct ΔH value of -2657.3 kJ, which matches the given energy release. Additionally, the coefficients in the balanced equation are consistent with the stoichiometry of butane combustion. Therefore, option e) is the correct answer.
In conclusion, the balanced equation for the combustion of butane is:
2C4H10(g) + O2(g) → 8CO2(g) + 10H2O(g) with a ΔH value of -2657.3 kJ.