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For question 1B on the 2010 final exam, could someone explain why it takes more heat to heat up 1 mole of butane gas than it does to heat up 1 mole of h2 gas from 10 to 20 degrees celsius? Also could someone explain the second part of question 1B?
For the second part of 1B, it is comparing a covalent bond( C-C is covalent because it shares its electrons) and a phase change ( such as melting ice which is solid ->liquid). Breaking a covalent bond would require more heat because you would need to break the chemical bond. A phase change does require a significant amount of heat in order to occur but it doesn't need to break any chemical bonds in the process so therefore it requires less heat than is needed to break a C-C bond.
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