A 25 g glass tumbler contains 400 mL of water at 24°C. If two 13 g...

A 25 g glass tumbler contains 400 mL of water at 24°C. If two 13 g ice cubes each at a temperature of -3°C are dropped into the tumbler, what is the final temperature of the drink? Neglect thermal conduction between the tumbler and the room.

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genius_generous answered 2 years ago

A 25 g glass tumbler contains 200 mL of water at 24°C. If two 15 g...

A 25 g glass tumbler contains 200 mL of water at 24°C. If two 15 g ice cubes each at a temperature of -3°C are dropped into the tumbler, what is the final temperature of the drink? Neglect thermal conduction between the tumbler and the room. 1°C

Consider a glass of 274 mL of water at 25°C. Calculate the mass of ice at...

Consider a glass of 274 mL of water at 25°C. Calculate the mass of ice at -15°C that must be added to cool the water to 10°C after thermal equilibrium is achieved. To find the mass of water use the density of water = 1.0 g/mL.

A calorimeter contains 20.0 mL of water at 12.5 ∘C . When 1.40 g of X...

A calorimeter contains 20.0 mL of water at 12.5 ∘C . When 1.40 g of X (a substance with a molar mass of 64.0 g/mol ) is added, it dissolves via the reaction X(s)+H2O(l)→X(aq) and the temperature of the solution increases to 28.5 ∘C . Calculate the enthalpy change, ΔH, for this reaction per mole of X. Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g⋅∘C)], that density of water is 1.00...

Part A A calorimeter contains 16.0 mL of water at 12.5 ∘C . When 1.70 g...

Part A A calorimeter contains 16.0 mL of water at 12.5 ∘C . When 1.70 g of X (a substance with a molar mass of 54.0 g/mol ) is added, it dissolves via the reaction X(s)+H2O(l)→X(aq) and the temperature of the solution increases to 30.0 ∘C . Calculate the enthalpy change, ΔH, for this reaction per mole of X. Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g⋅∘C)], that density of water...

PART A A calorimeter contains 27.0 mL of water at 14.5 ∘C . When 1.70 g...

PART A A calorimeter contains 27.0 mL of water at 14.5 ∘C . When 1.70 g of X (a substance with a molar mass of 75.0 g/mol) is added, it dissolves via the reaction X(s)+H2O(l)→X(aq) and the temperature of the solution increases to 28.5 ∘C . Calculate the enthalpy change, ΔH, for this reaction per mole of X. Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g⋅∘C)], that density of water is...

A calorimeter contains 31.0 mL of water at 15.0 ∘C . When 2.50 g of X...

A calorimeter contains 31.0 mL of water at 15.0 ∘C . When 2.50 g of X (a substance with a molar mass of 62.0 g/mol ) is added, it dissolves via the reaction X(s)+H2O(l)→X(aq) and the temperature of the solution increases to 28.5 ∘C . Calculate the enthalpy change, ΔH, for this reaction per mole of X. Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g⋅∘C)], that density of water is 1.00...

（1）A 31.5-g glass thermometer reads 24.1 ∘C before it is placed in 139 mL of water....

（1）A 31.5-g glass thermometer reads 24.1 ∘C before it is placed in 139 mL of water. When the water and thermometer come to equilibrium, the thermometer reads 41.8 ∘C. Ignore the mass of fluid inside the glass thermometer. The value of specific heat for water is 4186 J/kg⋅C∘, and for glass is 840 J/kg⋅C∘. Part A What was the original temperature of the water? （2） A crate of fruit with a mass of 37.0 kgkg and a specific heat capacity...

Part A: A calorimeter contains 18.0 mL of water at 13.5∘C. When 2.30 g of X...

Part A: A calorimeter contains 18.0 mL of water at 13.5∘C. When 2.30 g of X (a substance with a molar mass of 69.0 g/mol) is added, it dissolves via the reaction X(s)+H2O(l)→X(aq) and the temperature of the solution increases to 30.0∘C. Calculate the enthalpy change, ΔH, for this reaction per mole of X. Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g⋅∘C)], that density of water is 1.00 g/mL, and that...

19. The solubility of ammonium nitrate in water at 25°C is 118 g per 100 mL...

19. The solubility of ammonium nitrate in water at 25°C is 118 g per 100 mL of water and the density of a saturated aqueous solution of ammonium nitrate is 1.296 g/mL. Determine the concentration of a saturated aqueous ammonium nitrate solution in the following units. a) Molarity b) Molality c) Mole Fraction d) Weight Percent e) ppm 25. A 0.944 M solution of glucose in water has a density of 1.0624 g/mL at 20°C. What is the concentration of...

A 25 g piece of hot iron is dropped into a glass of ice water containing...

A 25 g piece of hot iron is dropped into a glass of ice water containing 15.0 g of ice and 50.0 g of water. If the iron loses 8.00 kJ of energy to the ice water in achieving equilibrium, what is the equilibrium temperature? ∆Hfus = 6.01 kJ/mol

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