An arctic explorer is trying to create drinking water by converting an ice ball into liquid. The ice ball has a mass of 225g and is at an initial temperature of -23C. The explorer heats the resulting water to a temperature of 37C. The heat of fusion of ice is 334J/g and the specific heat of ice is 2.1J/(g K). How much heat was required for the process?

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 25.09 g sample of a substance is initially at 24.0 °C. After absorbing 2121 J of heat, the temperature of the substance is 124.5 °C. What is the specific heat (?) of the substance?

4. Aluminum metal melts at 658.5°C. What would be the final temperature if 28.0 grams of solid aluminum at this temperature were placed into 520 grams of liquid aluminum at 1000.0°C? The heat of fusion for aluminum is 396 J/ -1 -1 g, and the specific heat of liquid aluminum is 0.481 J-g`¹deg-¹. (Note: this is the aluminum analog to the process you just did in lab!)

8. Heat is applied to 50g of water (specific heat of 4.18J/°C) at 25°C.  The temperature of the water increases to 98°C.  What was the total amount of heat energy that was applied?

A 35.0 g sample of bronze (specific heat: 0.402) is left in a deep freezer for several hours then placed into 75.5 g of water (specific heat: 4.184) initially at 25.0 ˚C. The water and the bronze stabilize when both are at 15.5 ˚C. What was the initial temperature of the bronze?

A sheet of metal weighing 275-g is heated to 100.0 °C and placed flat in 100.00 g bucket of water at 22.0 °C. What is the final temperature of the combined substances? Assume that no heat is lost to the surroundings. The specific heat capacity of the metal is 0.444 J/g.°C . The specific heat of water is 4.184 J/g.°C. Select one: O a. 61.0 °C Оъ. 82.4 °С O c. 79.2 °C d. 40.8 °C × О е. 39.6 °C

35 g of water at 40 C and 95 g of water at 60 C are mixed. What is the temperature of this mixture ? Specific heat capacity of water = 4.184 J/g.C. 58 C 48 C 55 C 45 C

A 20.25 g sample of a substance is initially at 28.9 °C. After absorbing 2217 J of heat, the temperature of the substance is 174.4 °C. What is the specific heat (?) of the substance?

When a 45.0 g sample of an alloy at 100.0 °C is dropped into 100.0 g of water at 25.0 °C, the final temperature is 37.0 °C. What is the specific heat of the alloy? The specific heat of H20(1) is 4.184 J'g-1.°c-1. q = mc AT O A. 0.423 J-g-1.°c-1 O B. 9.88 J-g-1.°C-1 O C. 48.8 J'g-1.°C-1 O D. 1.77 Jg-1.°c-1