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

Expert Solution

340 g ice will need = 340 g x 80 cal/g

= 27200 cal heat

360g melted Ice and 100g water to rise to

boiling temperature needs = 440 g x 100 cal/g

= 44000 cal

To boil off the whole amount need another = 440 g x 540 cal/g

= 237600 cal

Total heat needed = 27200 + 44000 + 237600

= 308800 cal = 3.1 x 10^5 cal

= 308.8 kcal

= 3.1 x 10^2 kcal

queen_honey_blossom answered 2 years ago

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...

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

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?

Part 1: A pot is made of 500 g steel with specific heat of 0.10 cal/(g °C). How much heat is needed to raise its temperature from 30 °C to 100 °C?

Part 1: A pot is made of 500 g steel with specific heat of 0.10 cal/(g °C). How much heat is needed to raise its temperature from 30 °C to 100 °C? Part 2: If we add 500 g of water into the pot above, how much heat is needed to raise the temperature of the pot of water from 30 °C to 100 °C? 2. A balloon shrinked to 90% of its orginal size after it was taken...

A handful of marshmallow (mass 5.00g, initial temperature 10.0 °C, specific heat as liquid 1.10 cal/g•K,...

A handful of marshmallow (mass 5.00g, initial temperature 10.0 °C, specific heat as liquid 1.10 cal/g•K, specific heat as solid 1.43 cal/g•K, latent heat of fusion 3.21 cal/g, melting temperature 45.0°C) is added to an insulated jug containing hot cocoa (mass 30.0g, initial temperature 93.0 °C, specific heat 0.380 cal/g•K). Find the final temperature of the cocoa-marshmallow mixture at equilibrium.

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...

Explain specific heat, latent heat of fusion and latent heat of vaporization. Write their mathematical relation...

Explain specific heat, latent heat of fusion and latent heat of vaporization. Write their mathematical relation and factors upon which it depends. (b) 3.5 kg ice is placed at initial temperature of −12°C. How much heat energy is required to convert this ice completely into steam

a) A 500.-g iceberg at -5.00°C is placed in a 226 g beaker with specific heat...

a) A 500.-g iceberg at -5.00°C is placed in a 226 g beaker with specific heat capacity 840 J/kg °C at temperature 15.0°C that contains 220 g of water. What is the minimum amount of steam needed to add into the system in order to melt the iceberg?

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?

Question