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 g/mL, and that no heat is lost to the calorimeter itself, nor to the surroundings.

Expert Solution

queen_honey_blossom answered 2 years ago

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 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...

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 200.0 g aluminum calorimeter contains 600.0 g of water at 20.0 °C. A 100.0 g...

A 200.0 g aluminum calorimeter contains 600.0 g of water at 20.0 °C. A 100.0 g piece of ice is cooled to −20.0 °C and then placed in the calorimeter. Use the following specific heats: cAl = 900.0 J Kg-1 °C-1, cwater = 4186 J Kg-1 °C-1, cice = 2.10 x 103 J Kg-1 °C-1. The latent heat of fusion for water is LF = 333.5 x 103 J/Kg. (a) Find the final temperature of the system, assuming no heat...

A 200 g aluminum calorimeter contains 500 g of water at 20 C. A 100 g...

A 200 g aluminum calorimeter contains 500 g of water at 20 C. A 100 g piece of ice cooled to -20 C is placed in the calorimeter. Find the final temperature of the system, assuming no heat losses. (The specific heat of ice is 2.0 kJ/kg K) A second 200 g piece of ice at -20 C is added. How much ice remains in the system after it reaches equilibrium? Would your answer to part b be different if...

When 50.0 mL of 60.0°C water was mixed in the calorimeter with 50.0 mL of 25.0°C...

When 50.0 mL of 60.0°C water was mixed in the calorimeter with 50.0 mL of 25.0°C water, the final temperature was measured as 40.8 °C. Assume the density for water is 1.000 g/mL regardless of temperature. a. Determine the magnitude of the heat lost by the hot water. b. determine the magnitude of the heat gained by the room temperature water. c. determine the heat gained by the calorimeter d. determine the calorimeter constant.

A coffee-cup calorimeter contains 130.0 g of water at 25.3 ∘C . A 124.0-g block of...

A coffee-cup calorimeter contains 130.0 g of water at 25.3 ∘C . A 124.0-g block of copper metal is heated to 100.4 ∘C by putting it in a beaker of boiling water. The specific heat of Cu(s) is 0.385 J/g⋅K . The Cu is added to the calorimeter, and after a time the contents of the cup reach a constant temperature of 30.3 ∘C . Part A Determine the amount of heat, in J , lost by the copper block....

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A coffee cup calorimeter contains 152.18 g of water at 20.90 °C. A 55.336 g piece of iron is heated to 98.37 °C. The piece of iron is added to the coffee cup caloriemter and the contents reach thermal equilibrium at 23.60 °C. The specific heat capacity of iron is 0.449 J g⋅K and the specific heat capacity of water is 4.184 J g⋅K . How much heat, q , is lost by the piece of iron? How much heat,...

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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