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?

Expert Solution

Energy required by the ice to completely melt, Qi = mCdT + mLf
Where m is the mass of ice, C is the specific heat of ice and Lf is latent heat of fusion of ice.
Qi = 500 x 2.04 x (5 - 0) + 500 x 334
= 172100 J

Energy given out as heat when glass and water is cooled to zero degree
Qf = Mw Cw dT + Mg Cg dT
= 220 x 4.186 x 15 + 226 x 0.84 x 15
= 16661.4 J

Cooling of glass and water takes off 16661.4 J of energy from ice
Remaining energy = 172100 J - 16661.4 J
= 155438.6 J
155438.6 = Mv Lv + Mv Cw dT
Where Mv and Lv are the mass and specific heat of vapour
= Mv [2230 + 4.186 x 100]
= Mv [2648.6]
Mv = 155438.6 / 2648.6
= 58.69 g

genius_generous answered 2 years ago

A 5.00 g sample of aluminum (specific heat capacity = 0.89 J °C-1 g-1) and a...

A 5.00 g sample of aluminum (specific heat capacity = 0.89 J °C-1 g-1) and a 10.00 g sample of iron (specific heat capacity = 0.45 J °C-1 g-1) are heated to 100.0 °C. The mixture of hot iron and aluminum is then dropped into 91.9 g of water at 23.7 °C. i) State the conditions for phase equilibrium of this system. NOTE: For an isolated system, the equilibrium state corresponds to the state with maximum entropy.

10.0 g of a substance at 60.0°C is placed into 20.0 g water at 5.00°C. The...

10.0 g of a substance at 60.0°C is placed into 20.0 g water at 5.00°C. The final temperature of both materials is 12.0°C. What is the specific heat of the unknown material?

determines the specific heat of the iron if 50 g of cloves are placed in 100...

determines the specific heat of the iron if 50 g of cloves are placed in 100 ml of cold water at 10º C and 100 ml of hot water at 70º C are added. The temperature of the mixture is 35.5ºC

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 tube is placed vertically in a beaker of salt water with a specific gravity of...

A tube is placed vertically in a beaker of salt water with a specific gravity of 1.15. The interfacial tension between the air and the water is 32 mN/m and the contact angle is 30 degrees, calculate: a) Capillary pressure in psi if the tube diameter is 0.0001 cm. b) Capillary rise of water in tube. c) If the cap rock thickness is 2ft, do you think this will stop water migration? d) Radius in inches of the largest pore,...

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

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...

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?

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.

Question