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- 1. Multiple ChoiceThe Law of Conservation of Energy states thatenergy is the capacity to do work.energy is neither created nor destroyed.heat flows from a warmer body to a cooler body.the total amount of energy in the universe is increasing.
- 2. Multiple ChoiceWhen a hydrocarbon is burned in the presence of oxygen, the amount of energy in the universeincreases.decreases.remains the same.cannot be determined without the specific heat of the hydrocarbon.
- 3. Multiple Choice
What energy transformation takes place when something burns?Chemical Potential → ThermalKinetic → Chemical PotentialElectromagnetic →
Chemical PotentialChemical Potential → Electrical - 4. Multiple ChoiceConsider the following specific heats:
Which substance, once warmed, would be more likely to maintain its heat and keep you warm through a long football game on a cold night?copperleadglasswater - 5. Multiple ChoiceCalculate the amount of heat absorbed in kilojoules to raise the temperature of a 79.0 g sample of ethanol from 298.0°C to 385.0°C. The specific heat capacity of ethanol is 2.42 J/g°C.16,600 kJ16.6 kJ-16,600 kJ-16.6 kJ
- 6. Multiple ChoiceA 6.50g sample of copper metal at 25.0°C is heated by the addition of 84.0 J of energy. The final temperature of the copper is ________°C. The specific heat capacity of copper is 0.38J/g·°C.29.99.059.034.0
- 7. Multiple ChoiceIt takes 11.2 kJ of energy to raise the temperature of 145 g of benzene from 23.0°C to 68.0°C. What is the specific heat of benzene?1.14 J/(g × °C)1.72 J/(g × °C)3.48 J/(g × °C)5.25 J/(g × °C)
- 8. Multiple ChoiceA piece of metal of mass 16.0 g at 107.0°C is placed in a calorimeter containing 50.0 g of water at 21.0°C. The final temperature of the mixture is 23.3°C. What is the specific heat capacity of the metal? Assume that there is no energy lost to the surroundings.0.36J/g°C2.8J/g°C0.18J/g°C4.2J/g°C
- 9. Multiple ChoiceA 25.0g piece of iron at 398K is placed in a styrofoam coffee cup containing 25.0 mL of water at 298 K. Assuming that no heat is lost to the cup or the surroundings, what will the final temperature of the water be? The specific heat capacity of iron = 0.449 J/g·K and water = 4.18 J/g·K.348 K308 K287 K325 K
- 10. Multiple Choice100.g of copper metal at 100°C is placed in 100.g of water at 20°C.
The specific heat of copper is 0.385J/g°C.
The specific heat of water is 4.18J/g°C.Heat is released by the copper metal.
The final temperature of the system will be closer to the initial temperature of the water.Heat is released by the water.
The final temperature of the system will be closer to the initial temperature of the water.Heat is released by the copper metal.
The final temperature of the system will be closer to the initial temperature of the copper metal.Heat is released by the water.
The final temperature of the system will be closer to the initial temperature of the copper metal. - 11. Multiple ChoiceHow many Joules are required to heat 2.0L of water in a pot from 20°C to the boiling point of water, 100°C? The specific heat of water is 4.18J/g°C and the density of water is 1.0g/mL.3.8x105J6.7x105J3.8x104J1.7x105J
- 12. Multiple ChoiceWhen a sample of a metal at 92°C is added to 43g of water at 20°C, the temperature of the water rises to 29°C. If the specific heat of the metal is known to be 0.952J/g°C and that of water is known to be 4.18J/g°C, what is the mass of the metal that was added to the water?43g54g27g12g
- 13. Multiple ChoiceA 0.80 g sample of sodium hydrogen carbonate was added to 50.0 mL of a 1.00 M HC2H3O2 solution and it was determined that 4,300J of energy was absorbed. Assume the density of the HC2H3O2(aq) is 1.0g/mL. Assume the specific heat of the solution to be 4.18 J/g°C. Calculate the temperature change in the calorimeter.20.3°C40.3°C10.3°C80.3°C
- 14. Multiple ChoiceA 4.20 g piece of magnesium ribbon was added to 100.0 mL of a 1.00 M HCl solution and it was determined that 6,800J of energy was released. Assume the density of the HCl(aq) is 1.0g/mL. Assume the specific heat of the solution to be 4.18 J/g°C. Calculate the temperature change in the calorimeter.45.6°C30.6°C15.6°C8.6°C
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