What is the change in entropy of 100 g of water when it is heated from...
What is the change in entropy when 2.00 kg of water at 100°C is heated to form steam at 100°C? 12 Now choose from one of the following options Why? a 2.42 x 107 J/K b) 1.21 x 107 J/K c 2.42 x 101 J/K 1.21 x 101J/K
1. a) Calculate the change in entropy (AS) when one mole of diamond is heated from a temperature of 0 K to 400 K at a constant pressure of 1 bar. The temperature-dependent heat capacity of diamond is C 2.9x10 T J/(mol K), where T is the absolute temperature in K. b) Given that the entropy of diamond is zero at 0 K, calculate its absolute molar entropy (S) at 400 K from the above result.
1. What is the change in entropy of 92.9 g of neon gas when it undergoes isothermal contraction from 20.1 L to 13.3 L? Assume ideal gas behavior. Enter a number to 2 decimal places. 2. Calculate the change in entropy in J/K for the melting of 12.0 g of ice at 0.0°C (ΔHfus = 6.02 kJ/mol). Enter a number to 2 decimals. 3. Calculate the entropy change when a 687 g sample of mercury is heated from 26°C to...
Calculate the change in entropy when one mole of metallic aluminum is heated at one bar pressure from an initial temperature of 25 °C to a final temperature of 750 °C. The molar heat capacities of solid and liquid aluminum at one bar pressure are 29.2 J mol' K and 31.75 J mol' K, respectively. The specific enthalpy of fusion of aluminum at its melting point (660.46 °C) is 396.57 J g! The molar mass of aluminum is 26.98 g...
Physical Chemistry Calculate the change in entropy when one mole of metallic aluminum is heated at one bar pressure from an initial temperature of 25 °C to a final temperature of 750 °C. The molar heat capacities of solid and liquid aluminum at one bar pressure are 29.2 J mol K1 and 31.75 J mol K, respectively. The specific enthalpy of fusion of aluminum at its melting point (660.46 °C) is 396.57 J g1. The molar mass of aluminum is...
The enthalpy of vaporization of water at 100 0°C is 40.43 kJ/mol. What is the entropy change in the surroundings when one mole of water vapor condenses at 100.0°C in a large room maintained at a temperature of 20.00°C? (answer in J/K) Answer Check
Calculate the change in entropy when one mole of metallic aluminum is heated at one bar pressure from an initial temperature of 25 ℃ to a final temperature of 750 ℃. The molar heat capacities of solid and liquid aluminum at one bar pressure are 29.2 J mol-1 K-1 and 31.75 J mol-1 K-1, respectively. The specific enthalpy of fusion of aluminum at its melting point (660.46 ℃) is 396.57 J g-1. The molar mass of aluminum is 26.98 g...
The enthalpy of vaporization of water at 100.0°C is 40.75kJ/mol. What is the entropy change in the surroundings when one mole of water vapor condenses at 100.0°C in a large room maintained at a temperature of 39.00°C? (answer in J/K) Answer: 131 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
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...