Calorimetry - Page 6
Questions
- If 65.34g piece of tin were to lose 754 Joules of energy in a calorimeter while experiencing a temperature change from 23.9 degrees C to 22.0 degrees C, how would you find its specific heat?
- How much heat do you need to raise the temperature of 150 g of ice from -30°C to -15°C?
- How do I find the change in temperature of #"199.0 g"# of water that loses #"2793 J"# of heat?
- The specific heat of silver is 0.24 J/g°C. How many joules of energy are needed to warm 7.37 g of silver from 25.0°C to 27.5°C?
- A 5.82-kg piece of copper metal is heated from 21.5°C to 328.3°C. What is the heat absorbed (in kJ) by the metal?
- How does differential scanning in calorimetry work?
- What is the total energy required to bring 3 kg ice from -10°C to 110°C?
- How many joules are required to increase the temperature of a 30.0 g block of gold from 25.0 ºC to 50.0 ºC? The specific heat of gold is 0.129 J/(g⋅°C) 4.184 J 96.8 J 193.5 J 3138 J
- The specific heat of ice is 0.492 cal/(g × °C). How many calories of heat are required to raise 100.0 g of ice from -20.0 °C to -0.5 °C?
- A 1.50-kg iron horseshoe initially at 600.0°C is dropped into a bucket containing 20.0 kg of water at 25.0°C. What is the final temperature?
- If the specific heat of water is 4.18J/g°C, how many joules of heat are given off when 5.0 g of water cool from 45°C to 25°C?
- How much energy is required to heat a #20*g# mass of ice, to give a #20*g# mass of steam at #120# #""^@C#?
- A sample of #H_2O# with a mass of 46.0 grams has a temperature of 100 °C. How many joules are necessary to boil the water? (use 2.0934 J/g for the heat of vaporization of water)
- How do I decide what mass and specific heat capacity to use to find the heat involved when I place a hot ionic solid into water? Do I use the mass of the solid or the water?
- How much heat is given off when a 24.7 kg iron ingot is cooled from 880°C to 13°C?
- Molten iron is extremely hot, averaging about 1,500°C The specific heat of iron is 0.46 J/g°C. How much heat is released to the atmosphere when 1 kg molten iron cools to room temperature (25°C)?
- 1. (a) A 300.0 g copper kettle contains 1.000 kg of water at 20.0 °C. How much energy must you supply to heat the kettle + water to 98.6 °C? (b) How much propane must you burn to provide this energy, if the transfer of the heat of combustion is 35 %?
- A sample of drinking water severely contaminated with chloroform , CHCl3 ,is supposed to be carcinogenic in nature . The level of combination was 15 ppm (by mass) .What is the molality of chloroform in the water sample ?
- What is the final temperature of 400 g of water at 20°C after it absorbs 226 kJ of heat?
- How much heat is required to heat a #10*g# mass of ice at #-10# #""^@C#, to give a #10*g# mass of water at #+10# #""^@C#?