
QUESTION 11 A 6.22g piece of metal at 97.6°C is placed in a calorimeter containing 25.0mL...
A 60.5 g sample of metal at 100°C is placed into a calorimeter containing 123 mL of water at 21.3 °C. After mixing the water/metal mixture reaches a temperature of 25.2 °C. Determine the specific heat of the metal in J/g°C. Assume the calorimeter absorbs a negligible amount of heat. Specific heat of water is 4.184 J/g°C
6. A piece of 155.0 g aluminium metal at 120°C was placed in a constant pressure calorimeter of negligible heat capacity containing 300.0 g of water at 20°C. Calculate the final temperature of the system (the aluminium metal and the water) in °C: given the specific heat of aluminium metal = 0.90 J/g °C, and that of water 4.184 J/g °C
QUESTION 19 A 63.1 g piece of metal whose T - 73.8 °C is placed in a coffee cup calorimeter containing 155 g water. When the system reaches equilibrium, the water has changed from 19.20 °C to 23.40°C. What is specific heat of metal? Density of water is 1.00 g/ml. Specific heat of H 20 is 4.184/gºo. 0.483 J/g °C 0.900 J/g °C 3.82 J/g °C 0.0150J/g °C 0.237 J/g °C 0.856 J/g °C 3.53 J/g °C 0.981 J/g °C
4. You placed 43.1 g of an unknown metal at 100 °C into a coffee cup calorimeter that contained 50.0 g of water that was initially at 22.0 °C. The equilibrium temperature of mixing (T0) was determined to be 23.7 °C. The calorimeter constant was known to be 51.5 J/°C. Specific HeatH2O = 4.184 J/g·°C a. What is the total amount of heat (J) lost by the metal? NG 1.5 b. What was the specific heat (J/g·°C) of the metal?...
A piece of metal weighing 5.50 g at a temperature of 34.5 °C was placed in a calorimeter in 32.35 mL of water at 22.5 °C. The final equilibrium temperature was found to be 27.5 °C. What is the specific heat of the metal? IVO AQ * R 0 O ? J/K-g
A 10.0 g piece of iron (C = 0.443 J/g oC) initially at 97.6 oC is placed in 50.0 g of water (C = 4.184 J/g oC) initially at 22.3 oC in an insulated container. The system is then allowed to come to thermal equilibrium. Assuming no heat flow to or from the surroundings, calculate the final temperature of the metal and water the change in entropy for the metal the change in entropy for the water the change in...
A piece of metal of mass 35.0 g at 100.0°C was placed in 150.0 g of water at 20.0 °C. After stirring, the final temperature of the water and the metal is 23.8°C. What is the specific heat capacity of the metal? (specific heat capacity for H2O = 4.184 J/g °C) O-0.89 J 8°C 19.6 J/g °C 1.96J/g °C O 0.89 J/g °C
A 10.95 g sample of lead at 88.0°C was placed into a styrofoam cup calorimeter which contained 15 mL of water at 22.0°C. The final temperature in the calorimeter reached 23.5°C. Calculate the specific heat of lead. The specific heat of water is 4.184 J/g°C.
A 70.0‑g piece of metal at 80.0 °C is placed in 100 g of water at 22.0 °C contained in a calorimeter. The metal and water come to the same temperature at 24.6 °C. How much heat did the metal give up to the water?
Question 22 (3 points) A 42.1 g piece of metal was heated to 95.4°C and then dropped into a beaker containing 42.0 g of water at 23.00°C. When the water and metal come to thermal equilibrium, the temperature is 32.10°C. What is the specific heat capacity of the metal? The specific heat capacity of the water is 4.184 J/(g-K) 0.387 J/(g-K) 0.600 J/(g-K) 0.488 J/(g-K) 0.720 J/(g-K) 0.980 J/(g-K)