12.0 g of aluminum at 200∘C and 22.0 g of copper are dropped into 50.0 cm3 of ethyl alcohol at 15.0∘C. The temperature quickly comes to 28.0 ∘C
What was the initial temperature of the copper in ∘C?
12.0 g of aluminum at 200∘C and 22.0 g of copper are dropped into 50.0 cm3...
11.0 g of aluminum at 200∘C and 22.0 g of copper are dropped into 44.0 cm3 of ethyl alcohol at 15.0∘C. The temperature quickly comes to 28.0 ∘C. What was the initial temperature of the copper in ∘C?
12.0 g of aluminum at 200∘Cand 18.0 g of copper are dropped into 43.0 cm3 of ethyl alcohol at 15.0∘C. The temperature quickly comes to 28.0 ∘C. What was the initial temperature of the copper in ∘C?
Physics 10.0 g of aluminum at 200Cand 22.0 g of copper are dropped into 53.0 cm3 of ethyl alcohol at 15.0 °C. The temperature quickly comes to 26.0°C What was the initial temperature of the copper in°C? Express your answer with the appropriate units. - 26.3 SubmitPrev Previous Answers Request Answer X Incorrect; Try Again; 3 attempts remaining
Can someone help me with these problems im stuck on? Thank you! 1) 2) Problem 12.88 Part A 0 g of aluminum at 200 °C and 20 g of copper are dropped into 43 cm3 of ethyl alcohol at 15 °C. The temperature quickly comes to 24 °C What was the initial temperature of the copper? Express your answer using two significant figures.
Go Far of the les in 1.4 g of hyd Update Problem 19.77 Review Part A 11.0 g of aluminum at 200 °C and 19.0g of copper are dropped into 43.0 em of ethyi alcohol at 15.0 C. The temperature quickly comes to 27.0 C What was the initial temperature of the copper in C? Express your answer with the appropriate units. Provide Feedback < Return to Assignment
10.0 g of aluminum at 2.00 × 102 °C and 20.0 g of copper are placed into a well-insulated container with 50.0 cm3 of ethanol at 21.0 °C. The combined system reaches an equilibrium temperature of 25.0 °C. Assume the temperature changes in the container itself can be safely ignored. What was the initial temperature of the copper?
A hot piece of aluminum weighing 50.0 grams at 350°C is dropped into 500. grams of water at 22.0°C. What is the final temperature of the water? The specific heat of aluminum is 0.902 J/g°C and that of water is 4.184 J/g°C.
A 400-g piece of copper, initially at 46.4°C, is dropped into 280 g of water contained in a 320 g aluminum can; the water and can are initially at 15.0°C. What is the final temperature of the system? (Specific heats of copper and aluminum are 0.092 and 0.215 cal/g · °C, respectively.) A) 16°C B) 18°C C) 24°C D) 26°C E) None of those answers
A 160 g block of aluminum heated to 120 °C is dropped into a 350 g copper calorimeter container containing 420 g of water. If the initial temperature of the calorimeter and the water is 25.0°C, what is the final equilibrium temperature of the system?
A copper block is removed from a 300°C oven and dropped into 1.00 kg of water at 20.0°C, which is located in an aluminum container of a mass of 0.250 kg. The system quickly reaches 25.5°, and then remains at that temperature. a) What is the mass of the copper block? b) How much energy did the copper block lose? c) How much energy did the water gain? d) As the temperature of water rises, the temperature of the copper...