What is the entropy change to the surroundings when 1 mol of ice melts in someone's hand if the hand temperature is 32°C? Assume a final temperature for the water of 0°C. The heat of fusion of ice is 6.01 kJ/mol. a. -188 J/K b. -22.0 J/K c. -19.7 J/K d. +19.7 J/K e. +188 J/K
What is the entropy change to the surroundings when 1 mol of ice melts in someone's...
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
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 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 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
1. Ice melts at 0C° with an enthalpy of fusion = 6.01 kJ mol-1 . An ice cube with a mass of 20.0g is placed inside an incubator at 40.0C°. Determine the total entropy change (in J/K) of this system. 2. Calculate the total entropy change (in J/K) when 50.0 g of H2 gas initially in a tank at a pressure of 145 psi is withdrawn from the tank under a constant pressure of 23.0 psi at standard room temperature....
1. loe melts at 0C with an enthalpy of fusion -6.01 kJ mol". An ice cube with a mass of 20.0g is placed inside an incubator at 40.0C°. Determine the total entropy change (in J/K) of this system.
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.
heat capacity of ?2?(?) 37.7 J/(mol⋅K) heat capacity of ?2?(?) 75.3 J/(mol⋅K) enthalpy of fusion of ?2? 6.01 kJ/mol Two 20.0‑g ice cubes at −14.0 °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.
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.
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.