An ice bag containing 0°C ice is much more effective in absorbing heat than one containing the same amount of 0°C water. The specific heat capacity of water is 1.00 kcal/(kg · °C), and its latent heat of fusion is 79.8 kcal/kg. (a) How much heat in kcal is required to raise the temperature of 0.500 kg of water from 0°C to 27.0°C?

How many joules are needed to change 50g of ice at 0°C to steam at 120°C?The latent heat of fusion of ice is 3.35 x 10°J/kg; latent heat of vaporization of water is 2.26 x 10°J/kg. The specific heat capacities of ice; water, and steam, respectively, are 2093 J/(kg. K), 4186 J/(kg. K) and 2010 J/(kg. K). out of Select one: A. 50.68 kJ B. 63.96 kJ O C. 227.6 kJ D. 53.96 kJ E. 20.5 kJ F. 800.2 kJ G. 153.7 kJ H. 22.76 kJ

Water with a mass of mW = 0.400 kg and temperature of TW = 19.5°C is poured into an insulated bucket containing mI = 0.19 kg of ice at a temperature of TI = -18.5°C. Assume the specific heats of ice and water are constant at cI = 2.10×103 J/(kg⋅°C) and cW = 4.19×103 J/(kg⋅°C), respectively. The latent heat of fusion for water is Lf = 334×103 J/kg.      Part (a)  What is the final temperature of the mixture, in degrees Celsius? Tfinal =          Part (b)  Enter an expression for the mass of ice, in kilograms, that has melted when the mixture reaches its final temperature. mmelt =     Part (c)  Calculate how much ice, in kilograms, has melted when the mixture reaches its final temperature. mmelt =

The fruit juice is heated in a heat exchanger using steam as a heating medium. The product flows through the heat exchanger at a rate of 1300 kg / hr and the intake temperature is 20 ° C. Determine the amount of steam required to heat the product to 100 ° C when only the latent heat of the vapor (assuming the inlet vapor temperature is equal to the temperature of the final product) is used for heating. The specific heat of the product is 4 kJ / (kg ° C). =

The specific heats of aluminum and iron are 0.214 and 0.107 calories per gram degrees Celsius​ [cal/(g °C​)] respectively. If we add the same amount of energy to a cube of each material​ (of the same​ mass) and find that the temperature of the aluminum increases by 27 degrees Fahrenheit ​[°F​], how much will the iron temperature increase in degrees Fahrenheit ​[°F​]?

Problem 6:   You have 4.9 kg of water in an insulated container. You add 0.95 kg of ice at -21 °C to the water and the mix reaches a final, equilibrium temperature of 11 °C. The specific heats of ice and water are 2.10 ×103 J/kg⋅C° and 4.19 ×103 J/kg⋅C°, respectively, and the latent heat of fusion for water is 3.34 ×105 J/kg.    Calculate the initial temperature of the water, in degrees Celsius.

A large jug containing 1.5kg of water is placed in the freezer. The water cools from 25°C to 0°C in a time of 60 minutes. The specific heat capacity of water is 4.2J/(g°C) (a) Calculate the thermal energy(heat) removed from the water as it cools from 25°C to 0°C.

The specific heat of most solids is nearly constant over a wide temperature range. Not so for diamond. Between 200 K and 600 K, the specific heat of diamond is reasonably well described by c=2.8T−350J/kg⋅K, where T is in K. For gemstone diamonds, 1 carat = 200 mg. How much heat energy is needed to raise the temperature of a 2.5 carat diamond from -50∘C to 250 ∘C?

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

You wish to cool a 1.95 kg block of brass initially at 80.0°C to a temperature of 41.0°C by placing it in a container of water initially at 20.0°C. Determine the volume (in L) of the liquid needed in order to accomplish this task without boiling. The density and specific heat of water are respectively 1,000 kg/m3 and 4,186 J/(kg · °C), and the specific heat of brass is 380 J/(kg · °C).