8. A 1.00 kg piece of aluminum (specific heat = 902 J/kg*C) originally at 90 degrees Celsius is placed in a container of water (specific heat = 4184 J/kg*C) originally at 25 degrees Celsius. The final temperature of the system is 40 degrees Celsius. What is the mass of the water in the container? (report your answer in kilograms to 3 decimal places)
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8. A 1.00 kg piece of aluminum (specific heat = 902 J/kg*C) originally at 90 degrees...
The value of specific heat for copper is 360 J/kg x C degrees, for aluminum is 900 J/kg x C degrees, and for water is 4186 J/kg x C degrees. Course Home <Ch 14 HW Item 6 6 of 10 Consta The value of specific heat for copper is 390 J/kg.C.for aluminun is 900 J/kg.C. and for water is 4186 J/kg.C. Part A What will be the equilibrium temperature when a 215 g block of copper at 235 °C is...
The specific heat of a particular substance is 147 J/(KC). Determine the latent heat of fusion of the substance if 1.64 kg of the substance at its melting point of -30,0 degrees Celsius, placed in a 0.631 kg aluminum container with 0.369 kg of water at 13.7 degrees Celsius results in an equilibrium temperature of 6.45 degrees Celsius. You don't need to
Calculate the specific heat of a metal from the following data. A container made of the metal has a mass of 3.6 kg and contains 14 kg of water. A 1.8 kg piece of the metal initially at a temperature of 180 degrees Celsius is dropped into the water. The container and water initially have a temperature of 16.0 degrees Celsius, and the final temperature of the entire (insulated) system is 18.0 degrees Celsius.
2 The specific heat of mercury is 138 J/kgC. The following is calorimeter data: 1.00 kg of solid HG at its melting point f-39.0 degrees C is placed in a 0.625 kg aluminum calorimeter with 0.400 kg of water at 12.80 C. The resulting equilibrium final temperature is 5.06 C. a. Draw the T-Q phase diagram that represents this b. Calculate the latent heat of fusion of mercury from this data. c. What is the change in entropy of the...
A piece of metal with a specific heat of 1.29 J/g°C is heated to 126.6°C and then placed in 133.868 g of water which is at a temperature of 10.9 °C. After a minute, the temperature of the water has stopped changing and is now 45.6°C. Assuming that there are no heat losses to the container or surroundings, what is the mass of the piece of metal in grams? Assume that water has a specific heat of 4.184 J/g°C. Enter...
The specific heat c is the amount of heat necessary to change the temperature of 1.00 kg of mass by 1.00°C. The specific heat c is a property of the substance; its Sl unit is J/(kg · K) or J/(kg.°C). Recall that the temperature change (AT) is the same in units of kelvin and degrees Celsius. water silver copper cup Case 1: A 0.780-kg silver pellet with a temperature of 85 °C is added to 0.150 kg of water in...
A piece of aluminum (specific heat 0.910kJ/kg 0C) of mass 193g at 71 0C is dropped into a Styrofoam cup filled with 121ml water at 20 0C. What are the final temperatures of the water and the aluminum? Please use C instead of 0C in your answer. Hint 1: because the cup is well-insulated, you can assume that all the heat leaving the aluminum as it cools goes to heating the water. Hint 2: How are the final temperature of...
What is the final temperature when 100 g of iron at 90 degrees Celsius is placed in 400 g of water at 25 degrees Celsius? The specific heat capacity of iron 0.45 J/g*K and the specific heat capacity of water is 4.184 J/g*K.
What is the final temperature when 100 g of iron at 90 degrees Celsius is placed in 400 g of water at 25 degrees Celsius? The specific heat capacity of iron 0.45 J/g*K and the specific heat capacity of water is 4.184 J/g*K
A 29 kg piece of zinc at 68◦C is placed in a container of water. The water had a mass of 28 kg and a temperature of 20◦C before the zinc was added. The specific heat of zinc and water are 388 J/kg ·◦ C and 4180 J/kg ·◦ C, respectively. What is the final temperature of water and zinc? Answer in units of ◦ C.