A student wants to measure the temperature change of water after adding a 5 cm3 block of copper to container 1 and a 20 cm3 block of copper to container 2. Both blocks of copper were heated to 40°C before they were added to the water. The image below shows the experiment immediately after adding the copper.What should be expected from this experiment? A. The temperature should increase more in container 2 because the 20 cm3 block contains more thermal energy. B. The temperature should decrease more in container 2 because the 20 cm3 block contains more thermal energy. C. The temperature should increase more in container 1 because the 5 cm3 block contains more thermal energy. D. The containers will have the same amount of temperature change because the 20 cm3 block and the 5 cm3 are made from the same element.

A student had a glass of water at 25°C. He put some ice in it. Once the ice melted, he found that the water's temperature had decreased to 18°C.The student puts the same amount of water at 25°C into another glass. He then adds more ice to this glass than he had added to the first glass. Which statement correctly explains what will happen after the ice melts? A. The water will be colder than 18°C because more thermal energy would have been added to it. B. The water will be warmer than 18°C because it would have received more heat from the ice. C. The water will be warmer than 18°C because melting would have taken place for a longer time. D. The water will be colder than 18°C because more heat would have flowed from it to the ice.

The temperature of 2.0 L of water is 42oC. Which would cause the temperature of the water to increase to 50oC?A.Removing thermal energy from the waterB.Adding water to increase the volumeC.Removing water to reduce the volumeD.Transferring thermal energy to the water

A chemist mixes 500 g of lead at 500°C with 1,200 g of water at 20°C. She then mixes 500 g of copper at 500°C with 1,200 g of water at 20°C. The specific heat capacity of lead is 0.1276 J/g°C and the specific heat capacity of copper is 0.3845 J/g°C. What will be true about the final temperatures of the two systems?  A. The final temperature of the lead-water system will be equal to the final temperature of the copper-water system.  B. The final temperature of the lead-water system will be higher than the final temperature of the copper-water system.  C. The final temperature of the lead-water system will be lower than the final temperature of the copper-water system.  D. Cannot be determined from the given information.

Calculate the energy needed to increase the temperature by 75 °C for 0.8 kg of copper.The specific heat capacity of copper is 385 J/kg°C.You must include units in your answer.

A 25.00 gram sample of an unknown metal initially at 99.0 degrees Celcius is added to 50.00 grams of water initially at 10.67 degrees Celcius. The final temperature of the system is 20.15 degrees Celcius. Calculate the specific heat of the metal. (The specific heat of water is 4.184 J/g*C).