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.)
8. Thermochemistry
Heat Capacity
Back8. Thermochemistry
Heat Capacity
- Multiple ChoiceA 28.5 g piece of gold is heated and then allowed to cool. What is the change in temperature (°C) if the gold releases 0.231 kJ of heat as it cools? The molar heat capacity of gold is 25.4 J/mol∙°C. (Atomic mass of gold = 197 g/mol)
- 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?
- Multiple ChoiceGiven that the heat of fusion of water is 6.02 kJ/mol, the heat capacity of H2O(l) is 75.2 J/mol·K, and the heat capacity of H2O(s) is 37.7 J/mol·K, calculate the total heat required to convert 1 mole of ice at -10°C to liquid water at 0°C.
- Multiple ChoiceHow much heat energy is required to melt 1 gram of ice at 0°C to liquid water at 0°C?
- Multiple Choice
Based on their given specific heat capacities which substance would show the greatest temperature change upon absorbing 25.0 J of heat?
8views - Open QuestionHow much heat is required to warm 1.50 kg of sand from 26.0 ∘c to 100.0 ∘c ?
- Multiple ChoiceHow much heat must be added to 25.0 g of water to raise the temperature from 15.0°C to 40.0°C? (Specific heat capacity of water is 4.18 J/g°C)
- 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.)
- Multiple ChoiceWhich of the following units correctly express specific heat capacity?
- Multiple ChoiceA volume of 75.0 mL of H2O is initially at room temperature (22.00 °C). A chilled steel rod at 2.00 °C is placed in the water. If the final temperature of the system is 21.10 °C, what is the mass of the steel bar? Use the following specific heat capacities: c_water = 4.18 J/g°C, c_steel = 0.452 J/g°C.
- 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?
- Multiple ChoiceHow much heat in joules is required to raise the temperature of a 100.0 g piece of copper from 18°C to 35°C, given that the specific heat capacity of copper is 0.385 J/g°C?
- Multiple ChoiceHow do you calculate the heat change when a solute with known mass is dissolved in water, considering its lattice energy and heat of hydration?
- Multiple ChoiceWhich has a greater heat capacity: iron or water?