A 150.0-g glass beaker contains 750 g of water initially at 25.0 degree C. A 250.0-g...
Suppose 0.385 kg of water initially at 39.5°C is poured into a 0.300 kg glass beaker having a temperature of 25.0°C. A 0.500 kg block of aluminum at 37.0°C is placed in the water, and the system insulated. Calculate the final equilibrium temperature of the system. °C
A 130 g copper bowl contains 210 g of water, both at 25.0°C. A very hot 450 g copper cylinder is dropped into the water, causing the water to boil, with 16.9 g being converted to steam. The final temperature of the system is 100°C. Neglect energy transfers with the environment. (a) How much energy is transferred to the water as heat? (b) How much to the bowl? (c) What is the original temperature of the cylinder? The specific heat...
please help me. Thanks A piece of copper metal weighing 36.3 g is initially at 100.0 degree C. It is dropped into a coffee cup calorimeter containing 50.0 g of water at a temperature of 20.0 degree C. After stirring, the final temperature of both copper and water is 25.0 degree C. Assuming no heat losses, an that the specific heat capacity of water is 4.184 J/g degreeC, what is the specific heat capacity of the copper in J/g degreeC?
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 hot lump of 35.6 g of copper at an initial temperature of 86.3 C is placed in 50.0 mL initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the copper and water, given that the specific heat of copper is 0.385 J/(gxC). Assume no heat is lost to surroundings.
21.A piece of copper metal is initially at 100 C. It is dropped into a coffee cup calorimeter containing 50.0g of water at a temperature of 20.0°C. After thermal equilibrium established, the final temperature of both copper and water is 25.0 °C. Assume there is no heat loss what is the heat capacity, C, of the copper? The specific heat of water is 4.18 J/g°C tutor a. 2.79 J/oC b. 3.33 JoC c. 2.79 J/oC d. 13.9 JoC 3
A piece of copper metal is initially at 83.0°C. It is dropped into a coffee cup calorimeter containing 30.0 9 of water at a temperature of 10.0°c. After stirring, the final temperature of both copper and water is 25.0°c. Assuming no heat losses, and that the specific heat (capacity) of water is 4.18 J/(g.), what is the heat capacity of the copper in J/K?
A copper vessel of mass 1000g contains 500g of water at 50C. An ice cube of mass 100g at temperature 30C is dropped into the vessel. a)Does the ice melt? Explain in a few words how you reached to your answer. b) What is the final temperature? c) Repeat part b if at the same time as dropping in the ice cube, wealso drop in a 200g piece of glass at a temperature of 110C. Specific heats in cal/g.C Ice=0.5...
A flask contains 150.0 g water at 35.00 °C. If you add 300.0 g iron at 350 °C to the flask and let the solution reach equilibrium, what is the final temperature of the water? c (water) = 4.184 J·g−1·°C−1, c (iron) = 0.450 J·g−1·°C−1.
A 400-g piece of copper, initially at 46.4°C, is dropped into 280 g of water contained in a 320 g aluminum can; the water and can are initially at 15.0°C. What is the final temperature of the system? (Specific heats of copper and aluminum are 0.092 and 0.215 cal/g · °C, respectively.) A) 16°C B) 18°C C) 24°C D) 26°C E) None of those answers