Multiple Choice
Why is it important that the thermometer does not touch the sides or bottom of the test tube when measuring temperature during an experiment involving thermal equilibrium?
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8. Thermochemistry
Thermal Equilibrium
Back8. Thermochemistry
Thermal Equilibrium
- Multiple ChoiceWhen water is heated in an insulated container and reaches thermal equilibrium with its surroundings, which of the following statements is true?16views
- Multiple ChoiceA 10.69-g block of solid platinum at 66.41°C is immersed in a 23.93-g pool of liquid ethanol with a temperature of 12.95°C. When thermal equilibrium is reached, what is the final temperature of the platinum and ethanol? Specific heat capacities: platinum = 0.133 J/g°C, ethanol = 2.44 J/g°C.261views
- Multiple ChoiceWhen ice is placed in hot water, what happens to the temperature of the ice and the water as they reach thermal equilibrium?25views
- Multiple Choice
If 53.2 g Al at 120.0 ºC is placed in 110.0 g H2O at 90 ºC within an insulated container that absorbs a negligible amount of heat, what is the final temperature of the aluminum? The specific heat capacities of water and aluminum are 4.184 J/g ∙ ºC and 0.897 J/g ∙ ºC, respectively.
2868views2rank4comments - Open Question
Suppose a 50.0 g block of silver (specific heat = 0.2350 J/g∙°C) at 100°C is placed in contact with a 50.0 g block of iron (specific heat = 0.4494 J/g∙°C) at 0°C, and the two blocks are insulated from the rest of the universe. the final temperature of the two blocks
600views - Multiple ChoiceA 14.4 g sample of granite initially at 75.0 °C is immersed into 30.0 g of water initially at 21.0 °C. Assuming the specific heat capacity of granite is 0.79 J/g°C, what is the final temperature of both substances when they reach thermal equilibrium?321views
- Multiple ChoiceA 140.0 g sample of water at 20.0 °C is mixed with 100.0 g of a certain metal at 95.0 °C. After thermal equilibrium is established, the temperature of the mixture is 24.6 °C. What is the specific heat capacity of the metal?262views
- Multiple ChoiceA 140.0 g sample of water at 20.0 °C is mixed with 100.0 g of a certain metal at 95.0 °C. After thermal equilibrium is established, the temperature of the mixture is 24.6 °C. What is the specific heat capacity of the metal?251views
- Multiple ChoiceA 2.10 g sample of lead, initially at 51.0 °C, is submerged into 76.1 g of water at 17.8 °C in an insulated container. What is the final temperature of both substances at thermal equilibrium? (The specific heat capacity of lead is 0.128 J/g°C and the specific heat capacity of water is 4.18 J/g°C.)179views
- Multiple ChoiceA 2.32 g lead weight, initially at 10.1 °C, is submerged in 7.61 g of water at 53.0 °C in an insulated container. What is the final temperature of both the weight and the water at thermal equilibrium?272views
- Multiple ChoiceA 2.54 g lead weight, initially at 10.3 °C, is submerged in 7.47 g of water at 52.5 °C in an insulated container. What is the final temperature of both substances at thermal equilibrium? Express the temperature in degrees Celsius.216views
- Multiple ChoiceA 32.8 g iron rod, initially at 22.8 °C, is submerged into an unknown mass of water at 64.0 °C, in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 59.5 °C. What is the mass of water?161views
- Multiple ChoiceA calorimeter contains 365 g of water at 30.0 °C. A 29.3-g sample of ice (at -11.0 °C) is added to the water in the calorimeter, and eventually all of the ice melts. Calculate the final temperature of the water. Assume no heat is lost to the calorimeter.220views
- Multiple ChoiceA 1.3 g wafer of pure gold initially at 69.8 °C is submerged into 64.1 g of water at 26.9 °C in an insulated container. The specific heat capacity for gold is 0.128 J/g°C and the specific heat capacity for water is 4.18 J/g°C. What is the final temperature of the system when thermal equilibrium is reached?198views