Calculate the change in entropy when 55 g of ice at 0 ℃ melts to water...

Question

Question

Calculate the change in entropy when 55 g of ice at 0 ℃ melts to water at 0 ℃? The heat of fusion is 3.34x10 5 J/kg.

Answer 1

Answer #1

Ans Mass of the ice a ma 55 gm. -0.055 kg a prouc 2273x, 3.34 x 10° T heat of fusion total heat energy required temper store

Answer 2

Similar Homework Help Questions

Calculate the change in entropy when 65 g of ice at 0 °C melts to water...

Calculate the change in entropy when 65 g of ice at 0 °C melts to water at 0 °C? The heat of fusion is 3.34x10 J/kg.
Please help 1. Calculate the increase of entropy (in J/K) when 42 g of ice melts...

Please help 1. Calculate the increase of entropy (in J/K) when 42 g of ice melts at 0 ºC and 1 atm. (The heat of fusion for ice is 6,000 J/mol.) 2. Calculate the change in entropy (in J/K) when a 34.0 g of water is heated from 12.4 ºC to 70.5 ºC at 1 atm. (The specific heat is 4.184 J/(g-K).) Notice that entropy and heat capacity have the same units.
Two kilograms of ice at 0 C melts to water at 0 C, and then is...

Two kilograms of ice at 0 C melts to water at 0 C, and then is heated to a temperature of 40 C. What is the change in entropy? You may assume the latent heat of fusion and specific heat for water is 3.35 x10^5 J/kg and 4186 J/KgK, respectively.

An ice tray contains 750g of liquid water at 0C. A) Calculate the entropy change of...

An ice tray contains 750g of liquid water at 0C. A) Calculate the entropy change of water as it is cooled slowly from 30C to 0C. B) Calculate the change in entropy of the water as it freezes slowly and completely at 0C. The heat of fusion of water is 3.33*10^5 j/kg
Calculate the change in entropy that occurs when 18.02 g of ice at –17.5°C is placed...

Calculate the change in entropy that occurs when 18.02 g of ice at –17.5°C is placed in 90.08 g of water at 100.0°C in a perfectly insulated vessel. Assume that the molar heat capacities for H2O(s) and H2O(l) are 37.5 J K^-1 mol^-1 and 75.3 J K^-1 mol^-1, respectively, and the molar enthalpy of fusion for ice is 6.01 kJ/mol. Change in entropy = ______J/K
What is the entropy change in the surroundings when one mole of ice melts at O.00C...

What is the entropy change in the surroundings when one mole of ice melts at O.00C in a large room maintained at 19.0C? The heat of fusion of ice is 6.11 kl/mol (answer in 3/) Answer Check

Calculate the entropy change when 72.00 g of ice, at 273.2 K and 1.000 bar pressure,...

Calculate the entropy change when 72.00 g of ice, at 273.2 K and 1.000 bar pressure, is melted and then heated to 298.2 K. The enthalpy of fusion of ice is 6.009 kJ/mole and the heat molar heat capacity of water at 1.000 atm is 75.43 J/ K mole Please help! Can't figure this homework problem out.
What is the entropy change in the surroundings when one mole of ice melts at 0.00°C...

What is the entropy change in the surroundings when one mole of ice melts at 0.00°C in a large room maintained at 19.0°C7 The heat of fusion of ice is 6.11 kl/mol. (answer in 1/K Answer: 22.4 Check
What is the entropy change in the surroundings when one mole of ice melts at 0.00'C...

What is the entropy change in the surroundings when one mole of ice melts at 0.00'C in a large room maintained at 27.0°C? The heat of fusion of ice is 6.31 kJ/mol (answer in 1/K) Answer: 21.0 Check Finis

Question 17 Not yet answered Calculate the increase of entropy (in J/K) when 73 g of...

Question 17 Not yet answered Calculate the increase of entropy (in J/K) when 73 g of ice melts at 0 °C and 1 atm. (The heat of fusion for ice is 6,000 J/mol.) Marked out of 1.00 Answer: P Flag question Calculate the change in entropy (in J/K) when 98.2 g of water is heated from 28.7 °C to 76.7 °C at 1 atm. (The specific heat is 4.184 J/(g-K).) Question 18 Not yet answered Marked out of 1.00 Notice...