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How much energy in kilojoules is required to convert 10.0 g of ice at -108 to water vapor at 1108°C? Specific heats are 2.09 J/g K for both ice and water vapor, and 4.18 J/g K for liquid water. Heats of vaporization and fusion are 2260 and 335 J/g.

This is what I did:

10g*108C*2.09J/g K + 10g * 335J/g + 10g*100C * 4.18 J/g K + 10g * 2260 J/g + 1008C * 10g * 2.09 J/g K= 50434.4 J =50.43 kJ

This question is a multiple choice, and there is no such choice, so this answer must be wrong. Unfortunately, I really don't know what is wrong with that.

I only the total energy is equal to the heat required to change the -108c ice to 0 C; then plus the energy require to melt the ice and then so far and so on....

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# Homework Help: Need help on a simple question-phase transfer

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