Cooking gas cylinders contain 92% butane (C4H10). Consider the following reaction.
C4H10(g) + 13/2 O2(g) → 4CO2 + 5H2O(l) △cH0 = –2655.0 kJ/mol
Which of the following statements are false?
a) when one mole of C4H10 is burned, four moles of CO2 are produced
b) when one mole of C4H10 is burned, 2655 kJ of energy are released
c) when one mole of C4H10 is burned, ten moles of H2O are produced
d) the reaction is endothermic
e) the reaction is a combustion
a) is true. According to the balanced equation, 1 mole of C4H10 reacts to produce 4 moles of CO2.
b) is true. According to the given ΔcH0 value, 2655 kJ of energy are released when one mole of C4H10 is burned.
c) is false. According to the balanced equation, 1 mole of C4H10 reacts to produce 5 moles of H2O.
d) is false. Endothermic reactions consume energy, while exothermic reactions release energy. Since energy is released in this reaction, it is exothermic.
e) is true. The reaction between C4H10 and O2 is a combustion reaction, as it involves the reaction of a hydrocarbon with oxygen to produce carbon dioxide and water.
which one is the correct false statement?
The correct false statement is c) when one mole of C4H10 is burned, ten moles of H2O are produced. According to the balanced equation, one mole of C4H10 reacts to produce 5 moles of H2O, not ten moles.
To determine which of the following statements are false, we need to analyze the given reaction equation and the information provided.
The balanced equation for the combustion of butane (C4H10) is:
C4H10(g) + 13/2 O2(g) → 4CO2 + 5H2O(l)
Statement a) When one mole of C4H10 is burned, four moles of CO2 are produced.
This statement is true, as the balanced equation shows that for every mole of C4H10, four moles of CO2 are produced.
Statement b) When one mole of C4H10 is burned, 2655 kJ of energy are released.
This statement is false. We are given the value of ΔcH0, which is the standard molar enthalpy of combustion. The negative sign indicates that the reaction is exothermic, meaning heat is released. However, the actual value of the energy released is not specified.
Statement c) When one mole of C4H10 is burned, ten moles of H2O are produced.
This statement is false. According to the balanced equation, when one mole of C4H10 is burned, only 5 moles of H2O are produced.
Statement d) The reaction is endothermic.
This statement is false. The given value of ΔcH0 is -2655.0 kJ/mol, indicating that the reaction is exothermic, not endothermic.
Statement e) The reaction is a combustion.
This statement is true. The given equation represents the combustion of butane. Combustion reactions involve the reaction of a substance with oxygen, resulting in the release of heat and the formation of carbon dioxide and water.
In summary, the false statements are:
b) when one mole of C4H10 is burned, 2655 kJ of energy are released
c) when one mole of C4H10 is burned, ten moles of H2O are produced
d) the reaction is endothermic