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The heats of fusion of three substances are listed below. Explain the trend this list reflects.
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Chapter 14 Solutions
Bundle: Introductory Chemistry: A Foundation, 8th + OWLv2 6-Months Printed Access Card
- A 0.250-g chunk of sodium metal is cautiously dropped into a mixture of 50.0 g water and 50.0 g ice, both at 0C. The reaction is 2Na(s)+2H2O(l)2NaOH(aq)+H2(g)H=368kJ Assuming no heat loss to the surroundings, will the ice melt? Assuming the final mixture has a specific heat capacity of 4.18 J/gc, calculate the final temperature. The enthalpy of fusion for ice is 6.02 kJ/mol.arrow_forwardThe following data are given for CC14: normalmeltingpoint=23Cnormalboilingpoint=77Cdensityofliquid=1.59g/mLvaporpressureat25C=110mmHg How much heat is required to vaporize 20.0 L of CCl4 at its normal boiling point?arrow_forwardWhich would you expect to have the higher fusion enthalpy, N2 or I2? Explain your choice.arrow_forward
- he enthalpy (H)of vaporization of water is about seven times larger than water’s enthalpy fusion(41kJ/molvs.6kJ/mol). What does this tell us about the relative similarities among the solid, liquid, and gaseous states of water?arrow_forwardWhat are the strongest attractive forces that must be overcome to (a) boil silicon hydride, SiH4? (b) vaporize calcium chloride? (c) dissolve Cl2 in carbon tetrachloride, CCl4? (d) melt iodine?arrow_forwardLiquid butane, C4H10, is stored in cylinders to be used as a fuel. Suppose 35.5 g of butane gas is removed from a cylinder. How much heat must be provided to vaporize this much gas? The heat of vaporization of butane is 21.3 kJ/mol.arrow_forward
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