Specific heat of ice: 2.09 J/(g⋅∘C Specific heat of liquid water: 4.18 J/(g⋅∘C) Enthalpy of fusion:...

Specific heat of ice: 2.09 J/(g⋅∘C
Specific heat of liquid water: 4.18 J/(g⋅∘C)
Enthalpy of fusion: ΔHfus=334J
Enthalpy of vaporization: ΔHvap=2250 J/g
How much heat energy, in kilojoules, is required to convert 47.0 g of ice at −−18.0 ∘C∘C to water at 25.0 ∘C?

Solutions

Expert Solution

Amanda K answered 4 months ago

Next > < Previous

Related Solutions

Given that the specific heat capacities of ice and steam are 2.06 J/g°C and 2.03 J/g°C,...

Given that the specific heat capacities of ice and steam are 2.06 J/g°C and 2.03 J/g°C, the molar heats of fusion and vaporization for water are 6.02 kJ/mol and 40.6 kJ/mol, respectively, and the specific heat capacity of water is 4.18 J/g°C, calculate the total quantity of heat evolved when 20.4 g of steam at 162°C is condensed, cooled, and frozen to ice at -50.°C.

Given that the specific heat capacities of ice and steam are 2.06 J/g°C and 2.03 J/g°C,...

Given that the specific heat capacities of ice and steam are 2.06 J/g°C and 2.03 J/g°C, the molar heats of fusion and vaporization for water are 6.02 kJ/mol and 40.6 kJ/mol, respectively, and the specific heat capacity of water is 4.18 J/g°C, calculate the total quantity of heat evolved when 13.2 g of steam at 192°C is condensed, cooled, and frozen to ice at -50.°C.

Given that the specific heat capacities of ice and steam are 2.06 J/g°C and 2.03 J/g°C,...

Given that the specific heat capacities of ice and steam are 2.06 J/g°C and 2.03 J/g°C, the molar heats of fusion and vaporization for water are 6.02 kJ/mol and 40.6 kJ/mol, respectively, and the specific heat capacity of water is 4.18 J/g°C, calculate the total quantity of heat evolved when 27.1 g of steam at 216°C is condensed, cooled, and frozen to ice at -50.°C. ______KJ Please show the steps

Take the heat capacity of ice as 2.108 J/(g*C) and the heat capacity of water as...

Take the heat capacity of ice as 2.108 J/(g*C) and the heat capacity of water as 4.184 J/(g*C) for this problem. For water, DHfus = 6.001 kJ/mol at 0 C. a. A 10.0 gram ice cube at -10.0 C is placed into 45.0 mL of water at 40 C. Determine the final physical state and temperature of the result. Calculate DS for the ice cube and the surrounding water, and Use the value DStot to explain why this process is...

1. Specific heat of water is 4.184 J/g ˚C. What is the heat in KJ gained...

1. Specific heat of water is 4.184 J/g ˚C. What is the heat in KJ gained when 20 q of water is heated from 22˚C to 77˚C? 2. What is the heat in J to melt 100g of NaCl when the HF for NaCl is 518 J/g? 3. What is the heat in J to equate 50 g Acetic Acid when the HE = 390 J/g?

The heat of fusion of ice is 80 cal/g at 0 °C and 1 atm, and...

The heat of fusion of ice is 80 cal/g at 0 °C and 1 atm, and the ratio of the specific volume of water to that of ice is 1.000:1.091. The saturated vapor pressure and the heat of vaporization of water at 0 °C are 6.026 × 10-3 atm and 600 cal/g, respectively. Estimate the triple point of water using these data

Water's heat of fusion is 80. cal/g , its specific heat is 1.0calg⋅∘C, and its heat...

Water's heat of fusion is 80. cal/g , its specific heat is 1.0calg⋅∘C, and its heat of vaporization is 540 cal/g . A canister is filled with 340 g of ice and 100. g of liquid water, both at 0 ∘C . The canister is placed in an oven until all the H2O has boiled off and the canister is empty. How much energy in calories was absorbed? Express your answer to two significant figures and include the appropriate units

Using the vlues for the heat of fusion, specific heat of water, and/or heat of vaporization,...

Using the vlues for the heat of fusion, specific heat of water, and/or heat of vaporization, calculate the amount of heat energy in each of the following: A) Kilocalories needed to melt a 525g ice sculpture at 0 degrees C and to warm the liquid to 15.o degrees C. B) Kilojoules released when 85.0g of steam condenses at 100 degrees C, cools ad freezes at 0 degrees C. Please show the formula and how so I can understand. For some...

Using the values for the heat of fusion, specific heat of water, and/or heat of vaporization,...

Using the values for the heat of fusion, specific heat of water, and/or heat of vaporization, calculate the amount of heat energy in each of the following: A. Joules released when 125g of steam at 100 C condenses and cools to liquid at 15.0 C. B. Kilocalories needed to melt a 525-g ice sculpture at 0 C and to warm the liquid to 15.0 C C. Kilojoules released when 85.0 g of steam condenses at 100 C, cools, and freezes...

Water's heat of fusion is 80. cal/g , and its specific heat is 1.0calg⋅∘C . Some...

Water's heat of fusion is 80. cal/g , and its specific heat is 1.0calg⋅∘C . Some velomobile seats have been designed to hold ice packs inside their cushions. If you started a ride with ice packs that held 1100 g of frozen water at 0 ∘C , and the temperature of the water at the end of the ride was 32 ∘C , how many calories of heat energy were absorbed? Express your answer to two significant figures and include...

Subjects