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A copper penny massing 2.49 g absorbs 32.1 J of heat. If its initial temperature was...
The specific heat of copper is 0.385 J/(g °C). If 34.2 g of copper, initially at 25°C, absorbs 7.880 kJ, what will be the final temperature of the copper? 25.4°C 598°C 27.8°C 623°C
4) A sample of 5.23 kg of copper absorbs heat, which raises the temperature 60.0°C. Determine the amount of heat absorbed, in kJ, if the specific heat capacity of aluminum is 0.385 J/gºC. (4 points)
4) A sample of 5.23 kg of copper absorbs heat, which raises the temperature 60.0°C. Determine the amount of heat absorbed, in kJ, if the specific heat capacity of aluminum is 0.385 J/gºC. (4 points)
It specific heat of copper is 0.385 J/(g.C). If 34.2 g of copper, initially at 24.0 C, absorbs 4.689 kJ, what will be the final temperature of the copper?
A sample of copper absorbs 43.6 kJ of heat, resulting in a temperature rise of 75.0 °C, determine the mass (in kg) of the copper sample if the specific heat capacity of copper is 0.385 J/g°C.
The specific heat of copper is 0.385 J/(g∙°C). If 34.2 g of copper, initially at 25°C, absorbs 4.689 kJ, what will be the final temperature of the copper? a. 25.4°C b. 27.8°C c. 356°C d. 381°C A chemical reaction causes the temperature of 1.0 x 102 g of water in a calorimeter to rise from 25°C to 40°C. The specific heat of water is 4.184 J/(g∙°C). What is the heat of reaction, qP? a. -0.31 kJ b. -0.75 kJ c....
The specific heat of copper is 0.385 J/(g∙°C). If 34.2 g of copper, initially at 25°C, absorbs 4.689 kJ, what will be the final temperature of the copper? a. 25.4°C b. 27.8°C c. 356°C d. 381°C A chemical reaction causes the temperature of 1.0 x 102 g of water in a calorimeter to rise from 25°C to 40°C. The specific heat of water is 4.184 J/(g∙°C). What is the heat of reaction, qP? a. -0.31 kJ b. -0.75 kJ c....
The initial temperature of 300.0 g of copper before it absorbs 1.850 kJ as heat was 25.0 ◦C. Find the final temperature of the copper
A hot lump of 27.4 g of copper at an initial temperature of 70.3 °C is placed in 50.0 mL of 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 0.385 J/(g·°C)? Assume no heat is lost to surroundings.
A hot lump of 30.9 g of copper at an initial temperature of 97.4 °C is placed in 50.0 mL of 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 0.385 J/(g·°C)? Assume no heat is lost to surroundings.