p (atm) 5 A 4 D B 1 → V (m³) 0 1 2 3 4 5 3. 2.

An aluminum plate has a circular hole. If the temperature of the plate increases, what happens to the size of the hole? 7.jpg Increases Decreases Stays the same Increases the top half of the hole More information is required

10. If it takes 554 calories to increase the temperature of 100 grams of a substance by 60.0 degrees Celsius then how many calories does it take to raise the temperature of 600 grams of the same substance by 60.0 degrees Celsius? No phase changes occur.   a. 13300   b. 554   c. 3324

2900000 48 cal/g eat meat sheet of paper, solve the following problems. Note that quantity of heat energy required to change the phase of a substance is given by the following equation: Q = mL, where is the heat required, m is the mass, and L is the heat of fusion or vaporization. 1. How much energy is absorbed when 25.0 g of ice at 0.0°C melts to form water at 0.0°C? The heat of fusion of ice is 80 cal/g. 2. How much energy is absorbed when the water at 0.0°C in Question 1 is heated to 100.0°C? The specific heat of water is 1.0 cal/g °C. 3. How much energy is absorbed when the water at 100.0°C in Question 2 vaporizes to 100.0°C? The heat of vaporization of water is 540 cal/g. 4. The steam in Question 3 is used to melt ice. How much ice will be melted by the energy released by the condensation of the steam at 100.0°C?

5 In order to determine the heat capacity of their latest phone, CrabappleTM engineers cool the phone in the freezer to -31.7ºC. They then drop it into a calorimeter with some water in it that is at a temperature of 50.8ºC. The calorimeter (including the water) has a total heat capacity of 869.42 J/ºC. After a few minutes the temperature of the calorimeter is stabilized to 31ºC. What is the heat capacity of the phone? Enter your answer with at least 3 sig figs assuming units of J/ºC.

Problem 6:  Suppose you pour 0.0125 kg of 20.0°C water onto a 1.1-kg block of ice, sitting in a large bowl, which is initially at -15.0°C. The latent heat of fusion for water is Lf = 334 kJ/kg.   What is the final temperature of this system? You may assume that the water cools so rapidly that effects of the surroundings are negligible.

1) Listen How much energy would have to be added to 519grams of water to heat it from 17.0°C to 84.0°C? O 3.53x105 J O 1.46x108 J O 6.95x104 J O7.39x105 J O7.39x108 J O 1.46x105 J

€2 When an air bubble rises from the bottom to the top of a freshwater lake, its volume increases by 75%. If the temperature at the bottom of the lake was 3°C and at the top was 13.5°C, how deep is the lake? Hint The lake is Question Help: Message instructor Submit Question #3 3 E 80 F3 $ 4 F4 R cr dº % m deep. 5 F5 T A 6 MacBook Air F6 & 7 F7 Y U *00 8 DII F8 - ( 9 DD F9 1 0 0

A copper sample (ccu = 387 J/kg•K) of mass mẹ = 75 g and temperature Te = 312ºC is dropped into a glass beaker that contains a mass of water me = 220 g (cw = 4190 J/kg•K). %3D The initial temperature of the water and the beaker is Tw,b = 12.0°C. What is the final temperature of the copper, beaker, and water? * The heat capacity (the specific heat times the mass) of the beaker is Cb' = 190 J/K.

QUESTION 7 The average body temperature of a living human being is 98.6° F. This temperature in kelvins is а. 300 K b. 310 K C. 293 K d. 273 K е. 283 К