Calculate the final temperature (Tf) when 45.0 g of Hg receive 50.0 J of heat (q)...
The specific heat of copper is 0.385 J/gC . Calculate the final temperature when 25.0 g of copper metal at 100C is added to 50 mL of water at 20 C
A hot lump of 42.0 g of aluminum at an initial temperature of 90.5 °C is placed in 50.0 mL H2O initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the aluminum and water, given that the specific heat of aluminum is 0.903 J/(g·°C)? Assume no heat is lost to surroundings.
Calculate the final temperature of 6.84 g of praseodymium (specific heat capacity = 0.193 J g-1 °C-1) initially at 26.8 °C that releases 11.3 J of energy into the surroundings. A)14.3°C B)18.2 °C C)21.6 °C D)23.8 °C E)8.17 °C
4. Calculate the heat change in a system (q) when 12.0 g of water is heated from 20.0 °C to 100.0 °C. 5. A 295 g aluminum engine at an initial temperature of 3.00 °C absorbs 85.0 kJ of heat. What is the final temperature of the engine? The specific heat capacity for aluminum is 0.900 J/(g K).
Calculate the amount of heat (in loules) that must be added to 50.0 g of water to increase the temperature from 26.3C to 52.70. The specific heat of water is 4.18 J/g C An 50.0 g iron nail was heated in a blacksmith forge until it glowed cherry red. It was then dropped into a calorimeter containing 50.0 g of water at room temperature (21.5°C) and swirled gently until the temperature reached its maximum. The final temperature was 26.0 C....
A hot lump of 32.3 g of copper at an initial temperature of 96.5°C is placed in 50.0 mL H2O 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 0.385J/g°C and the specific heat of water is 4.184J/g°C? 4. A hot lump of 32.3 g of copper at an initial temperature of 96.5°C is placed in 50.0 mL H20 initially at 25.0°C...
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.
4. Heat transfer: q = mass x Cs x ΔT and –qreaction = +qsolution a. A piece of metal with a mass of 8.6 g was heated to 100.0°C and dropped into a coffee cup calorimeter containing 402.4 g of water at 25.0°C. If the temperature of the water and the metal at thermal equilibrium is 26.4°C, what is the specific heat of this metal in J/g°C? b. How much heat energy must be added in order to boil a...
Calculate the final temperature for each of the following mixtures. Assume no heat loss to the environment. Show your method for part b. 50.0 g of water at 25.0 degree C is mixed with 50.0 g of water at 85.0 degree C. 75.0 g of water at 25.0 degree C is mixed with 25.0 g of water at 85.0 degree C. In Part B of this experiment, 0.10 g of Mg is added to 50. mL of 1.0M HCl. Which...
521.8 J of heat was added to 8.00 g of water. The final temperature of the water was measured to be 64.2oC. What was the initial temperature of the water? (specific heat capacity of water = 4.184 J/goC)