Multiple Choice
Which best explains why water has a high specific heat?
8. Thermochemistry
Heat Capacity
Back8. Thermochemistry
Heat Capacity
- Multiple ChoiceWhat is the amount of energy required to raise the temperature of one gram of water by 1°C?
- Multiple ChoiceWhat is the amount of heat required to raise the temperature of water by one degree Celsius referred to as?
- Multiple ChoiceWhich amount of energy is required to raise the temperature of one gram of water by one degree Celsius?
- Multiple ChoiceWhich of the following helps most to explain why water has a high specific heat?
- Multiple ChoiceHow much heat, in kJ, is required to warm 1.59 L of water from 23.7 °C to 79.5 °C? The specific heat of water is 4.184 J/g°C. Assume a density of 1.00 g/mL for water.
- Multiple Choice
50.00 g of heated metal ore is placed into an insulated beaker containing 822.5 g of water. Once the metal heats up the final temperature of the water is 32.08 ºC. If the metal gains 14.55 kJ of energy, what is the initial temperature of the water?
- Multiple Choice
A sample of copper absorbs 3.53 kJ of heat, which increases the temperature by 25 ºC, determine the mass (in kg) of the copper sample if the specific heat capacity of copper is 0.385 J / g ºC.
- Multiple Choice
Based on their given specific heat capacities which substance would show the greatest temperature change upon absorbing 25.0 J of heat?
- Multiple ChoiceWhich of the following exchanges of energy has a positive sign for heat (relative to the system)?
- Open Question
If 14.5 kJ of heat were added to 485 g of liquid water, how much would its temperature increase?
- Open Question
The temperature of the cooling water as it leaves the hot engine of an automobile is 240 °F. After it passes through the radiator it has a temperature of 175 °F. calculate the amount of heat transferred from the engine to the surroundings by one gallon of water with a specific heat of 4.184 J/g °C.
- Open QuestionWhich sample is most likely to undergo the smallest change in temperature upon the absorption of 100 kj of heat?
- Open QuestionHow much heat is required to warm 1.50 kg of sand from 26.0 ∘c to 100.0 ∘c ?
- Multiple ChoiceA 1.05 x 10^3 g piece of iron (specific heat = 0.499 J g^-1 °C^-1) is dropped into 0.652 kg of water, and the water temperature rises from 24.9°C to 35.2°C. What must have been the initial temperature of the iron? Specific heat of water is 4.18 J g^-1 °C^-1.