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.
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
3 answers
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.