10.0 g of a substance at 60.0°C is placed into 20.0 g water at 5.00°C. The...

10.0 g of a substance at 60.0°C is placed into 20.0 g water at 5.00°C. The final temperature of both materials is 12.0°C. What is the specific heat of the unknown material?

Expert Solution

Specific heat for unknown material is found to be 1.225 J /g °C

queen_honey_blossom answered 2 years ago

Two 20.0-g ice cubes at –20.0 °C are placed into 225 g of water at 25.0...

Two 20.0-g ice cubes at –20.0 °C are placed into 225 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature of the water after all the ice melts.

Suppose 28.0 g of ice at -10.0∘C is placed into 300.0 g of water in a...

Suppose 28.0 g of ice at -10.0∘C is placed into 300.0 g of water in a 200.0-g copper calorimeter. The final temperature of the water and copper calorimeter is 18.0∘C. 1) What was the initial common temperature of the water and copper? (Express your answer to three significant figures.)

Two 20.0 g ice cubes at −11.0 ∘C are placed into 225 g of water at...

Two 20.0 g ice cubes at −11.0 ∘C are placed into 225 g of water at 25.0 ∘C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, Tf, of the water after all the ice melts. heat capacity of H2O(s)H2O(s) 37.7 J/(mol⋅K) heat capacity of H2O(l)H2O(l) 75.3 J/(mol⋅K) enthalpy of fusion of H2OH2O 6.01 kJ/mol Tf= ∘C

Two 20.0-g ice cubes at –21.0 °C are placed into 295 g of water at 25.0...

Two 20.0-g ice cubes at –21.0 °C are placed into 295 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature of the water after all the ice melts. heat capacity of H2O(s) 37.7 heat capacity of H2O (l) 75.3 enthalpy of fusion of H2O 6.01

Two 20.0-g ice cubes at –19.0 °C are placed into 245 g of water at 25.0...

Two 20.0-g ice cubes at –19.0 °C are placed into 245 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, Tf, of the water after all the ice melts. Heat capacity of H20(s) = 37.7J/(mol*K) Heat cap of H20(l) 75.3 J/(mol*K) enthalpy of fusion of H20 = 6.01 kJ/mol

Two 20.0-g ice cubes at –16.0 °C are placed into 275 g of water at 25.0...

Two 20.0-g ice cubes at –16.0 °C are placed into 275 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature of the water after all the ice melts. Given the Following Values: Heat Capacity of H2O (s) = 37.7 J/mol*K Heat Capacity of H2O (l) = 75.3 J/mol*K Enthalpy of Fusion of H2O = 6.01 kJ/mol

Two 20.0-g ice cubes at –19.0 °C are placed into 215 g of water at 25.0...

Two 20.0-g ice cubes at –19.0 °C are placed into 215 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature of the water after all the ice melts.

Two 20.0-g ice cubes at –21.0 °C are placed into 225 g of water at 25.0...

Two 20.0-g ice cubes at –21.0 °C are placed into 225 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature of the water after all the ice melts.

Two 20.0 g ice cubes at −12.0 ∘C are placed into 255 gof water at 25.0...

Two 20.0 g ice cubes at −12.0 ∘C are placed into 255 gof water at 25.0 ∘C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, Tf, of the water after all the ice melts.

An aqueous solution of 0.0190g of a protein in 10.0 mL of water at 20.0 ̊C...

An aqueous solution of 0.0190g of a protein in 10.0 mL of water at 20.0 ̊C shows a 5.22 cm rise inthe apparatus shown in the figure. Assume the density of the solution to be 0.998g/mL, andthe density of mercury to be 13.6 g/cm3. What is the molar mass of the protein?

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