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?
12.0 g of aluminum at 200∘Cand 18.0 g of copper are dropped into 43.0 cm3 of...
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 19.0 g of copper are dropped into 50.0 cm3 of ethyl alcohol at 15.0∘C. The temperature quickly comes to 28.0 ∘C. Part A What was the initial temperature of the copper in ∘C? Express your answer with the appropriate units.
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?
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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
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
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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.
A 43.0-g sample of copper at 99.9 °C is dropped into a beaker containing 149 g of water at 18.2 °C. What is the final temperature when thermal equilibrium is reached? (The specific heat capacities of liquid water and copper are 4.184 J/g · K and 0.385 J/g · K, respectively.) Final temperature = How much energy is required to raise the temperature of 14.7 grams of gaseous hydrogen from 24.7 °C to 37.7 °C ? Answer: Joules.
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
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 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?