57.8 g iron at 12.6°C is placed in thermal contact with 43.5 g iron at 49.5°C. What is the final temperature?
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57.8 g iron at 12.6°C is placed in thermal contact with 43.5 g iron at 49.5°C....
A metal sample weighing 43.5 g and at a temperature of 100.0 °C was placed in 39.9 g of water in a calorimeter at 25.1 °C. At equilibrium the temperature of the water and metal was 33.5 °C. 1. What is the unknown metal?
uestion 2 When 49.5 J of heat was transferred to 7.3 g iron at 22°C, the temperature of iron increases to 37°C. What is the specific heat of iron in yg ?C? 045 O 0.45 22 24 None of these
A metal sample weighing 43.5 g and at a temperature of 100.0 °C was placed in 39.9 g of water in a calorimeter at 25.1 °C. At equilibrium, the temperature of the water and metal was 33.5 °C. Determine the specific heat capacity of the metal.
A 4.31 kg block of Copper at +275oC is placed into thermal contact with a block of ice at +0.000oC. When they reach thermal equilibrium, the final temperature of everything is 0.000oC and only HALF of the ice has melted into water! What was the original amount of ice (in kg)?
A hot lump of 42.5 g of iron at an initial temperature of 98.4 °C is placed in 50.0 mL of H2O initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the iron and water given that the specific heat of iron is 0.449 J/(g·°C)? Assume no heat is lost to surroundings.
A hot lump of 30.9 g of iron at an initial temperature of 86.4 °C is placed in 50.0 mL H, initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the iron and water, given that the specific heat of iron is 0.449 J/(g.°C)? Assume no heat is lost to surroundings.
A 1.5g iron nail is heated to 95.0 *C and placed into a beaker of water. Calculate the heat gained by the water if the final equilibrium temperature is 57.8 *C. Thespecific heat capacity of iron= 0.449 J/g *C; of water= 4.18 J/g *C.Choose the answer from the following but show work.a.) 6.0 Jb.) 25 Jc.) -25 Jd.) 39 Je.) -39 Jwould you please show how you came up with the answer, THANKS.
A metal sample weighing 43.5 g at a temperature of 100.0 °C was placed in 39.9 g of water in a calorimeter at 25.1°C. At equilibrium, the temperature of the water and metal was 33.5°C. What was ΔT for the water? (ΔT = Tfinal - Tinitial) What was ΔT for the metal? Using the specific heat of water (4.184 J/g°C), calculate how much heat flowed into the water. Calculate the specific heat of the metal.
3. A 100 g block of copper initially at 60°C is placed in contact with a 300 g block of aluminum initially at 30°C in an insulated container. A. Identify the block that loses thermal energy. (5 pts) B. Calculate the final equilibrium temperature of the two blocks. (15 pts) Copper a(Cu) = 17 x 10-61°C Ccu = 0.0923 cal/g.K = 386 J/kg-K LF (Cu) = 207 kJ/kg
A 150.0 g block of iron absorbs 750.0 J of thermal energy. The specific heat capacity of iron is 0.449 J/(g·◦C). The initial temperature of the block is 20.0 ◦C. What is its final temperature? (A) 111.3 ◦C (B) 31.1 ◦C (C) 22.2 ◦C (D) 20.4 ◦C (E) 8.86 ◦C