b=765.00 C    Hvap=889.6 j/g tm=321.00c     Hfus=54.40 j/g specific heat solid=0.2300 J/g  specific heat liquid = 0.2640 j/g  A 47.30 g sample of liquid cadmium at 390.00°C is poured into a mold and allowed to cool to 21.00°C. How many kJ of energy are released in this process?

Solve the following problems following the method shown above. Useful Information: Specific heat of water, H20() = 4.18 J/g-"C Specific heat of ice, H20(s) = 2.04 J/g.C Specific heat of steam, H2O(g) = 2.00 J/g.C Heat of fusion of ice (0°C) = 334 J/g Heat of vaporization of water (100°C) = 2260 J/g Heat of condensation of water = 2260 J/g 4. Calculate the number of joules needed to turn 325 grams of water at 100°C to steam at 100°C. 5. Calculate the heat released when 875 grams of water at 0.0°C turns to ice at 0.0°C. 6. Calculate the number of joules needed to vaporize 2.00 x 102 grams of liquid ammonia at its boiling point and produce ammonia vapor at the same temperature. The heat of vaporization of liquid ammonia is 1374 J/g. 7. How much heat is needed to melt 25.4 g of iodine? Hr = 61.7 J/g. 8. How much heat is needed to melt 4.24 g of Pd? Hr = 162 J/g.

If the same amount of heat is added to 5.00 g samples of each of the metals below, which metal will experience the largest temperature change?   Metal Specific Heat Capacity (J/g-K) A 0.753 B 0.129 C 0.385 D 0.449 E 0.897

What is the identity of a 10.0 solid metal sample that has its temperature increased by 14.0°C when q = 53.9 J of heat energy was absorbed? Metal sample: Au: 0.128 Ag: 0.235 Cu: 0.385 Fe: 0.449 Al: 0.903