A copper kettle weighs 1.09 kg. (The specific heat of copper is 0.384 J/g·°C) (a) What is the heat capacity (in J/°C) of the kettle? (b) How much heat (in J) is required to increase the temperature of this kettle from 23.2°C to 98.5°C?   (c) How much heat (in J) is required to heat this kettle from 23.2°C to 98.5°C if it contains 1.04 L of water (density of 0.997 g/mL and a specific heat of 4.18 J/g·°C across the temperature range)?

In the laboratory a student finds that it takes 21.8 Joules to increase the temperature of 13.1 grams of solid tungsten from 24.9 to 38.3 degrees Celsius. The specific heat of tungsten calculated from her data is J/g°C.

2. A small immersion heater was used to heat water in an insulated cup. The heater was placed in 100.0 g of distilled water initially at 21.0°C, and turned on for 60.0 seconds while the water was stirred with a thermometer. The final temperature of the water was measured to be 37.5°C. Assume the specific heat capacity of the water is 4.18 J/g °C. (a) Calculate the total heat energy in joules absorbed by the water and the average power in watts (1 watt = 1 joule/s) delivered by the heater. The heater was used to deliver 3000 joules of energy to 100.0 g of methanol (CH,OH(E)) in the same manner. The temperature of the methanol increased by 11.8 Celsius degrees. (b) Calculate the specific heat capacity of the methanol liquid. (c) (i) Calculate the mass of water (H,O, Co= 4.181 Jgl °C-) at 20.0°C that would be requireć %3D to cool a 30.0-g block of copper (Cu, co0.385 J gl °C-l) from 50.0°C to 25.0°C in an insulated cup. %3D (ii) Which liquid, water or methanol, would be more effective as…

The initial temperature of a 415 g sample of iron is 10.6 °C. If the sample absorbs 2.64 kJ of energy as heat, what is its final temperature? The heat capacity of iron is 0.449 J/(g · °C).