Multiple Choice
How much energy is required to vaporize 10.00 grams of water at its boiling point (100 °C)? (The enthalpy of vaporization of water at 100 °C is 40.7 kJ/mol.)
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8. Thermochemistry
Heat Capacity
Back8. Thermochemistry
Heat Capacity
- Multiple ChoiceHow much heat energy is required to melt 1 gram of ice at 0°C to liquid water at 0°C?16views
- Multiple ChoiceIf 14.5 kJ of heat is added to 485 g of liquid water, how much will the temperature of the water increase? (Assume the specific heat capacity of water is 4.18 J/g·°C.)18views
- Multiple ChoiceWhich of the following units correctly express specific heat capacity?27views
- Multiple ChoiceIf 400 J of energy is added to 10 grams of water (specific heat capacity = 4.18 J/g·°C), what is the resulting temperature change?31views
- Multiple ChoiceWhich has a greater heat capacity: iron or water?36views
- 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.
3555views13rank - Multiple Choice
Based on their given specific heat capacities which substance would show the greatest temperature change upon absorbing 25.0 J of heat?
3005views11rank3comments - Multiple ChoiceWhich of the following exchanges of energy has a positive sign for heat (relative to the system)?740views
- Open Question
If 14.5 kJ of heat were added to 485 g of liquid water, how much would its temperature increase?
922views - 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.
602views - Open QuestionWhich sample is most likely to undergo the smallest change in temperature upon the absorption of 100 kj of heat?813views
- Open QuestionHow much heat is required to warm 1.50 kg of sand from 26.0 ∘c to 100.0 ∘c ?710views
- 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^-1.337views
- Multiple ChoiceA 10.5-g ice cube at 0°C is placed onto a 245-g block of aluminum. Calculate the temperature change of the aluminum upon the complete melting of the ice. Assume that all of the energy required to melt the ice comes from the aluminum. The specific heat capacity of aluminum is 0.897 J/g°C and the heat of fusion of ice is 334 J/g. What is the temperature change of the aluminum?232views