How many grams of copper can be cooled from 66.8 to 20.3 °C by the heat...
How many grams of copper can be cooled from 66.8 to 20.3 °C by
the heat gained by 100.0 g of water that has an increase in
temperature from 24.7 to 33.6 °C?
Answer in joules and in calories
Homework Answers
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How many grams of copper can be cooled from 66.8 to 20.3 °C by
the heat...
20. How many grams of water can be cooled from 35 to 20 °C by evaporation of 60 grams of water? (heat of vaporizati...
20. How many grams of water can be cooled from 35 to 20 °C by evaporation of 60 grams of water? (heat of vaporization of water = 2.4 kJ/g) (specific heat of water = 4.18J/mole K) A) 1.6 x 10 g B) 2.3 x 103g C) 2.6 g D) 1.6 g E) 2.3 g
a) how many joules are needed to heat up 325 grams of water from 25.1 degrees c to 43.8 degrees c? how many calories? b)...
a) how many joules are needed to heat up 325 grams of water from 25.1 degrees c to 43.8 degrees c? how many calories? b) how many joules are needed to heat up 325 grams of aluminum from 25.1 degrees c to 89.5 degrees c? how many calories? the c for aluminum is = 0.897 j/g degrees c
Part 1: Specific Heat of Copper Metal Your Data Neighbor 1 Neighbor 2 Weight of copper...
Part 1: Specific Heat of Copper Metal Your Data Neighbor 1 Neighbor 2 Weight of copper taken, grams 24.724 g __ 24.916 g 25.124 g Weight of water taken, grams 49.591 g_ 50.129 g 24.983 g Temperature of heated copper, 100°C 100°C 100°C Temperature of cool water, °C 22°C 23.2°C 21.5°C Final temperature reached, °C 25.5°C 26.5°C 24.9°C Heat GAINED by water, Joules Heat LOST by copper, Joules Specific heat of copper, Joules/g°C Average value of specific heat of copper...
A 43.0-g sample of copper at 99.9 °C is dropped into a beaker containing 149 g...
A 43.0-g sample of copper at 99.9 °C is dropped into a beaker containing 149 g of water at 18.2 °C. What is the final temperature when thermal equilibrium is reached? (The specific heat capacities of liquid water and copper are 4.184 J/g · K and 0.385 J/g · K, respectively.) Final temperature = How much energy is required to raise the temperature of 14.7 grams of gaseous hydrogen from 24.7 °C to 37.7 °C ? Answer: Joules.
A copper block with a mass of 500 grams is cooled to 77 K by being...
A copper block with a mass of 500 grams is cooled to 77 K by being immersed in liquid nitrogen. The block is then placed in a Styrofoam cup containing some water that is initially at +50.0°C. Assume no heat is transferred to the cup or the surroundings. The specific heat of liquid water is 4186 J/(kg °C), of solid water is 2060 J/(kg °C), and of copper is 385 J/(kg °C). The latent heat of fusion of water is...
A copper block with a mass of 600 grams is cooled to 77K by being immersed...
A copper block with a mass of 600 grams is cooled to 77K by being immersed in liquid nitrogen. The block is then placed in a Styrofoam cup containing some water that is initially at +50.0°C. Assume no heat is transferred to the cup or the surroundings. The specific heat of liquid water is 4186 J/(kg °C), of solid water is 2060 J/(kg °C), and of copper is 385 J/(kg °C). The latent heat of fusion of water is 3.35...
Find the mass HomeworkUnanswered A copper block with a mass of 700 grams is cooled to...
Find the mass HomeworkUnanswered A copper block with a mass of 700 grams is cooled to 77K by being immersed in liquid nitrogen. The block is then placed in a Styrofoam cup containing some water that is initially at +50.0°C. Assume no heat is transferred to the cup or the surroundings. The specific heat of liquid water is 4186 J/(kg °C), of solid water is 2060 J/(kg°C), and of copper is 385 J/(kg °C). The latent heat of fusion of...
Perd cific Zinc has a specific heat of 0.39 J/g °C while iron has a spe-...
Perd cific Zinc has a specific heat of 0.39 J/g °C while iron has a spe- cific heat of 0.45 J/g °C. If a 100-g sample of each metal is cooled from 100 °C to room temperature (25 °C), which one releases more heat energy? 50. Th deg ab 10 51. An engineer tests the thermal properties of a metal alloy. Using a 50.0-g sample, she finds that adding 485 J of heat energy to the alloy causes a temperature...
o prase Ul Water to 2. What is the heat, q, required to melt 10 grams...
o prase Ul Water to 2. What is the heat, q, required to melt 10 grams of ice in a) Joules b) calories? 122.3 °C). The goC. Assuming -4.18 /(8°C) 3. A piece of metal weighing 49.047 g was heated to 100.0 °C and then put it into 100.0 m water initially at 22.3 °C). The metal and water were allowed to come to an equilibu temperature, determined to be 27.8 °C. Assuming no heat lost to the environment, calculat...
a) A 430 mL sample of water was cooled from 100.0 oC to 30.0 oC . How much...
a) A 430 mL sample of water was cooled from 100.0 oC to 30.0 oC . How much heat was lost? b) How many kilojoules are required to change the temperature of 26.5 g of water from 19.8 oC to 29.0 oC ? c) Calculate the final temperature when 10 mL of water at 80 oC are added to 20 mL of water at 25 oC d) A piece of metal weighing 2.00 g at a temperature of 41.0 oC was placed in a calorimeter in 19.10 mL of water...
20. How many grams of water can be cooled from 35 to 20 °C by evaporation of 60 grams of water? (heat of vaporization of water = 2.4 kJ/g) (specific heat of water = 4.18J/mole K) A) 1.6 x 10 g B) 2.3 x 103g C) 2.6 g D) 1.6 g E) 2.3 g
Part 1: Specific Heat of Copper Metal Your Data Neighbor 1 Neighbor 2 Weight of copper taken, grams 24.724 g __ 24.916 g 25.124 g Weight of water taken, grams 49.591 g_ 50.129 g 24.983 g Temperature of heated copper, 100°C 100°C 100°C Temperature of cool water, °C 22°C 23.2°C 21.5°C Final temperature reached, °C 25.5°C 26.5°C 24.9°C Heat GAINED by water, Joules Heat LOST by copper, Joules Specific heat of copper, Joules/g°C Average value of specific heat of copper...
A 43.0-g sample of copper at 99.9 °C is dropped into a beaker containing 149 g of water at 18.2 °C. What is the final temperature when thermal equilibrium is reached? (The specific heat capacities of liquid water and copper are 4.184 J/g · K and 0.385 J/g · K, respectively.) Final temperature = How much energy is required to raise the temperature of 14.7 grams of gaseous hydrogen from 24.7 °C to 37.7 °C ? Answer: Joules.
Find the mass HomeworkUnanswered A copper block with a mass of 700 grams is cooled to 77K by being immersed in liquid nitrogen. The block is then placed in a Styrofoam cup containing some water that is initially at +50.0°C. Assume no heat is transferred to the cup or the surroundings. The specific heat of liquid water is 4186 J/(kg °C), of solid water is 2060 J/(kg°C), and of copper is 385 J/(kg °C). The latent heat of fusion of...
Perd cific Zinc has a specific heat of 0.39 J/g °C while iron has a spe- cific heat of 0.45 J/g °C. If a 100-g sample of each metal is cooled from 100 °C to room temperature (25 °C), which one releases more heat energy? 50. Th deg ab 10 51. An engineer tests the thermal properties of a metal alloy. Using a 50.0-g sample, she finds that adding 485 J of heat energy to the alloy causes a temperature...
o prase Ul Water to 2. What is the heat, q, required to melt 10 grams of ice in a) Joules b) calories? 122.3 °C). The goC. Assuming -4.18 /(8°C) 3. A piece of metal weighing 49.047 g was heated to 100.0 °C and then put it into 100.0 m water initially at 22.3 °C). The metal and water were allowed to come to an equilibu temperature, determined to be 27.8 °C. Assuming no heat lost to the environment, calculat...
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