Chapter 12, Question 11 Ice melts at 273.15 K with ΔHfus = 6.01 kJ/mol. An ice cube of mass 34.4 g is dropped into a swimming pool, the temperature of which is held at 27.2°C.
(a) What is the entropy change (ΔS) for melting the ice?
ΔS = ------J/K
(b) What is ΔS of the pool?
ΔS = ------J/K
(c) What is the overall ΔS?
ΔS = ------J/K
Chapter 12, Question 11 Ice melts at 273.15 K with ΔHfus = 6.01 kJ/mol. An ice...
Chapter 12, Question 11 Your answer is partially correct. Try again. Ice melts at 273.15 K with AHfus = 6.01 kJ/mol. An ice cube of mass 23.1 g is dropped into a swimming pool, the temperature of which is held at 22.7°C. (a) What is the entropy change (AS) for melting the ice? as = T28. 23 J K (b) What is AS of the pool? 0.428 AS = J/K (c) What is the overall AS? 28.65 AS = J/K...
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.
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 Calculate the total entropy change (in J/K) when 50.0 g of H2 gas initially in a tank at a pressure of 145 psi is withdrawn from the tank under a constant pressure of 23.0 psi at standard room temperature....
A substance melts with an enthalpy change of 75 kJ/mol and an entropy change of 98 J/K.mol. What is its melting temperature? A) 0.77 K B) 765 K C) 1.69 K D) 425 K E) 591 K
Property Value Units Melting point 0 °C Boiling point 100.0 °C ΔHfus 6.01 kJ/mol ΔHvap 40.67 kJ/mol cp (s) 37.1 J/mol · °C cp (l) 75.3 J/mol · °C cp (g) 33.6 J/mol · °C Based on the thermodynamic properties provided for water, determine the energy change when the temperature of 0.750 kg of water decreased from 115 °C to 43.0 °C.
The enthalpy of fusion of H2O (s) (ice) if heat fusion= 6.01 kj mol-1. What mass (ink) of ice can be melted with the heat released from the combustion of 1.00 gallon of octane? ( The temperature of the ice and resulting water remains constant at 0 degrees C through the melting process.) Please show work
You have a block of ice at a temperature of -100°C. This block of ice is made from 180g H2O. The block of ice will be heated continually until it becomes super-heated steam at a temperature of 200°C Cice = 2.03 J/g-K ΔHfus=6.01 kJ/mol Cwater = 4.18 J/g-K Csteam = 1.84 J/g-K ΔHvap=40.67 kJ/mol What is the enthalpy change raising the temperature of 180 g of ice at −100 °C to 0°C? What is the enthalpy change upon melting 180...
1. Ice (1.0 kg) at -10.0 °C is allowed to melt and warm to 25.0 °C, under isobaric conditions (1 bar). Considering the ice/water as the system, calculate the entropy changes for both the system and the surroundings. What is the overall change in entropy? Over the temperature ranges considered, the heat capacities of ice and water can be considered constant, at 36.9 J mol-1 K-1 for ice and 75.29 J mol-1 K-1 for water at 1 bar. The enthalpy...
Calculate the enthalpy change upon converting 1.00 mol of ice at -25 °C to steam at 125 °C under a constant pressure of 1 atm. The specific heats of ice, liquid water, and steam are 2.03, 4.18, and 1.84 J/g-K, respectively. For H2O, ΔHfus = 6.01 kJ/mol and ΔHvap=40.67 kJ/mol.
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.