An insulated Thermos contains 128 g of water at 81.3 ˚C. You put in a 12.5...

An insulated Thermos contains 128 g of water at 81.3 ˚C. You put in a 12.5 g ice cube at 0.00 ˚C to form a system of ice + original water. The specific heat of liquid water is 4190 J/kg•K; and the heat of fusion of water is 333 kJ/kg. What is the net entropy change of the system from then until the system reaches the final (equilibrium) temperature?

Expert Solution

genius_generous answered 1 year ago

An insulated Thermos contains 145 g of water at 70.7 ˚C. You put in a 11.0...

An insulated Thermos contains 145 g of water at 70.7 ˚C. You put in a 11.0 g ice cube at 0.00 ˚C to form a system of ice + original water. The specific heat of liquid water is 4190 J/kg•K; and the heat of fusion of water is 333 kJ/kg. What is the net entropy change of the system from then until the system reaches the final (equilibrium) temperature?

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...

An 13 g ice cube at -13˚C is put into a Thermos flask containing 110 cm3...

An 13 g ice cube at -13˚C is put into a Thermos flask containing 110 cm3 of water at 18˚C. By how much has the entropy of the cube-water system changed when a final equilibrium state is reached? The specific heat of ice is 2200 J/kg K and that of liquid water is 4187 J/kg K. The heat of fusion of water is 333 × 103 J/kg.

An 7.5 g ice cube at −10°C is put into a Thermos flask containing 150 cm3...

An 7.5 g ice cube at −10°C is put into a Thermos flask containing 150 cm3 of water at 21°C. By how much has the entropy of the cube–water system changed when equilibrium is reached? The specific heat of ice is 2220 J/kg · K. (The latent heat of fusion for water is 333 kJ/kg.)

An 8.5 g ice cube at −10°C is put into a Thermos flask containing 150 cm3...

An 8.5 g ice cube at −10°C is put into a Thermos flask containing 150 cm3 of water at 30°C. By how much has the entropy of the cube-water system changed when equilibrium is reached? The specific heat of ice is 2220 J/kg · K. (The latent heat of fusion for ice is 333 kJ/kg and the specific heat of water is 4187 J/kg · K.)

A 200 g insulated aluminum cup at 16 ∘C is filled with 255 g of water...

A 200 g insulated aluminum cup at 16 ∘C is filled with 255 g of water at 100 ∘C a) Determine the final temperature of the mixture. b) Determine the total change in entropy as a result of the mixing process (use ΔS=∫dQ/T).

A 65 g ice cube at 0 °C is placed in an insulated box that contains...

A 65 g ice cube at 0 °C is placed in an insulated box that contains 8 g of steam at 200 °C. What is the equilibrium temperature reached by this closed system? Approximate the specific heat capacity of steam to be 1.5 J/g oC. All the other values can be found on the textbook. [Note: Assume that all of the steam condenses.]

A 50·g ice cube (at 0°C) is placed in an insulated cup with 250·g of water...

A 50·g ice cube (at 0°C) is placed in an insulated cup with 250·g of water which is at 46°C. The latent heat of fusion for ice is 80·cal/g and the specific heat of water is 1.0·cal/g/°C. (a) How much heat will the ice have to absorb from the water to completely melt (and turn into 0°C water)? ___ cal. (b) Find the temperature of the 250·g of water initially at 46°C after it loses the heat required to melt...

A thermos contains 150cm3 of coffee at 85◦C. To cool the coffee, you drop two 11g...

A thermos contains 150cm3 of coffee at 85◦C. To cool the coffee, you drop two 11g ice cubes into the thermos. The ice cubes are initially at −10◦C and melt completely. What is the final temperature of the coffee? Treat the coffee as if it were water. Cice =2×103J/kg/◦C, CH2O =4186J/kg/◦C, Lf H2O =3.35×105J/kg.

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