When you turn your hot water on in the shower, it takes a bit for the water to get warm. Some of this is because the water in the pipe is cold but some of it is because the water from the hot water heater must heat the copper plumbing pipe itself. Copper has a specific heat of 0.39ER. How much energy does it take to heat 2 kilograms of copper pipe from 70°F to 130°F? Report your answer in Joules. (Hint: Note that you'll need to convert kJ to J and F to K.)

To determine the specific heat of an object, a student heats it to 100 ∘C∘C in boiling water. She then places the 55.4 gg object in a 179 gg aluminum calorimeter containing 129 gg of water. The aluminum and water are initially at a temperature of 19.9 ∘C∘C, and are thermally insulated from their surroundings. If the final temperature is 22.3 ∘C∘C, what is the specific heat of the objectand the type of material?

Geologists measure conductive heat flow out of the earth by drilling holes (a few hundred meters deep) and measuring the temperature as a function of depth. Suppose that in a certain location the temperature increases by 20°C per kilometer of depth and the thermal conductivity of the rock is 2.5 W/m·K. What is the rate of heat conduction per square meter in this location? Assuming that this value is typical of other locations over all of earth's surface, at approximately what rate is the earth losing heat via conduction? (The radius of the earth is 6400 km.)

An ice tray is removed from a freezer, where the ice was at a temperature of -11°C, and left on a countertop. If the mass of the ice is 0.29 kg, how much heat must be added in k to turn all the ice into room temperature water (that is, liquid water at 20°C)? The specific heat of water is 4.2 kgC kJ the heat of fusion of water is 335 kg kJ and the specific heat of ice is 2.1 kg°C* 133.69 This is a change of phase question. There are 3 cases we have to consider: 1. The heat required to increase the temperature of the ice, Q1 2. The heat required to turn the ice into a liquid (a phase change), Q2 3. The heat required to raise the temperature of the now liquid water, Q3 For Q1, you will use the equation Q = mcATusing the c=2.1 kJ/(kg*C). Keep in mind that the hp

In an effort to stay awake for an all-night study session, a student makes a cup of coffee by first placing a 220-W electric immersion heater in 0.320 kgm of water. (a) How much heat must be added to the water to raise its temperature from 20.0 °C to 80.0°C? (b) How much time is required? Assume that all of the heater's power goes into heating of water.

An ice bag containing 0°C ice is much more effective in absorbing heat than one containing the same amount of 0°C water.   (a) How much heat (in J) is required to raise the temperature of 0.900 kg of water from 0°C to 25.0°C?   (b) How much heat (in J) is required to first melt 0.900 kg of 0°C ice and then raise its temperature?   (c) Explain how your answers support the contention that the ice is more effective.

@ 2 O: F2 W S 8. An electric immersion heater has a power rating of 1900 W. If the heater is placed in a 1.8 kg of water at 30 °C, how many minutes will it take to bring the water to a boiling temperature? (Assume that there is no heat loss except to the water itself. Cwater=4186 J/kg.°C) min # 3 X 80 F3 E D $ 4 C F4 R TI F or do % 5 V F5 T G > 6 MacBook Air B F6 < H 887 & ◄◄ F7 U N * 8 J DII F8 M ( 9 K F9 O ) C L F10 (4) P F11 31 + 11 F12 18 BEL ?

A bullet made of silver (specific heat 234 J/kg deg C) traveling at 380 m/s hits a wooden post and stops. If 39% of the kinetic energy of the bullet becomes heat trapped in the bullet, what is the temperature change (in deg C) of the bullet? (Hint: you do not need the mass of the bullet, it cancels out)

A small electric immersion heater is used to heat 82 g of water for a cup of instant coffee. The heater is labeled “150 watts” (it converts electrical energy to thermal energy at this rate). Calculate the time required to bring all this water from 25°C to 100°C, ignoring any heat losses. (The specific heat of water is 4186 J/kg·K.)

1.2-kg of ice at -6.0°C is dropped into 5.0 L (5.566-kg) of car coolant. The initial temperature of the coolant is 25.0°C. The ice and coolant are insulated, so energy transfers to the outside is negligible. After hours, all ice melts and the final temperature of the mixture of water-coolant is 1.8°C. The specific heat of ice is 2090 J/kg °C; the specific heat of water is 4186 J/kg °C; the latent heat of fusion for water is 334000 J/kg. A. What is the energy needed for heating the ice to 0 °C? B. Determine the energy needed to melt the ice into water. C. Determine the total energy needed to heat the -6.0°C ice to 1.8°C water. (Please note: the total energy also includes the part heating water from 0.0 °C to 1.8 °C.) D. Determine the specific heat capacity of the coolant.