22. Using the following data for water, determine the energy required to melt 1.

Question

22. Using the following data for water, determine the energy required to melt 1.00 mole of ice (solid water at its melting Boiling point 373 K Melting point 273 K Enthalpy of vaporization 2,260 J/g Enthalpy of fusion 334 J/g Specific heat capacity (solid) 2.11 J/(g K) Specific heat capacity (liquid) 4.18 J/ Specific heat capacity (gas) 2.08 J/ a. 11.7 kJ d. 23.2 kJ b. 4.96 kJ e. 2.26 kJ c. 6.02 kJ 23. Which of the following hydrocarbons has the greatest fuel value? d. 6H12 a. C5H12 b. C7H16 e. C6Hi4 c. C10H

Explanation / Answer

22. 1 mole of ice

Mole=weight/Molecular weight

1=X/18

weight of Ice= 18 Gr

The molar heat of fusion=6.02 kj/mol

therefore enrgy= 6.02 kj

23. Answer is a

Pentane has great fuel value than remaining

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