The specific heat of solid copper is 0.385 J/(g·°C). A) What thermal energy change occurs when the temperature of a 27.00  g sample of copper is cooled from 34.00 °C to 14.00 °C?  Be sure to give your answer the proper sign. B) The above calculation indicates the amount of heat used to melt solid ice at 0°C. The molar heat of fusion of ice is 6.00 kJ/mol. How many moles of ice are melted?

What quantity of heat (in KJ) will be absorbed by a 59.9 g piece of aluminum (specific heat equals 0.930J/G. As it changes temperature from 23.0°C to 67.0°C.

4. An ice cube at a temperature of -4.0°C has a mass of 7.0 g. You add 150. mL of hot water (90.0°C) to the ice cube. The water cools to 50.00°C. Calculate the heat of fusion (Q) in kJ and the enthalpy of fusion (AH) in kJ/mol.

A 251 g piece of lead (SH=0.160 J/g degrees Celsius) with an initial temperature of 90.5 degrees Celsius is placed in 100.0 mL of water with an initial temperature of 21.5 degrees Celsius. What is the temperature of the water at equilibrium? How much heat in joules was transferred from the metal to the water?

A 28.5 g piece of gold is heated and then allowed to cool. What is the change in temperature (°C) if the gold releases 0.220 kJ of heat as it cools? The molar heat capacity of gold is 25.4 J/mol °C.

Use the information provided below to calculate the quantity of heat (in kJ) required to convert 63.01 g of substance A from an initial temperature of 54.44°C to a final temperature of -6.64°C. The molar mass of the substance is 27.1 g/mol. Melting Point of A = 1.686°C Heat of fusion = 11.19 kJ/mol Boiling point of A 108.5°C Heat of vaporization = 71.95 kJ/mol %3D Solid Liquid Gas Specific heat (J/g°C) 2.89 4.14 6.42 Report your answer to the tenths place and do not include units. Do not include a sign with your answer.

12. When freezing weather threatens the citrus crop in Florida, growers spray their orange trees with water, using their knowledge of enthalpy to protect the fruit. How much heat is released when 1000 g of liquid water at 10.0°C is completely converted to ice of a temperature of -2.0°C? A. 8.2 x 104 J B: 6.1 x 105 J C. 3.3 x 105 J D.) 3.8 x 10³ J E. 4.2 x 104 J

The specific heat capacity of silver is 0.24 J/g°C. Calculate the specific heat capacity of silver in cal/g°C.

What is the specific heat of silver if it requires 86.3 J of energy to raise the temperature of 15.0 g of silver 25°C a) 4.3 J/g °C b) 0.23 J/g °C c) 0.14 J/g °C d) 0.60 J/g °C

A sample of 175°C copper is placed into a beaker with 100 grams of 25°C water. Which sample of copper will heat the water to the lowest final temperature? The specific heat of copper is 0.385 J-g-1.°C-1. The specific heat of water is 4.184 J·g-1.°C-1. A. 5.0 g Cu B. 2.0 g Cu C. 0.5 g Cu D. 1.0 g Cu