Question

Ice at 0.0 °C is used to cool water. What is the minimum mass of ice required to cool 325 g of water from 30.5 °C to 4.0 °C? (Heat of fusion = 333 J/g; specific heat capacities ice = 2.06 J/gK, liquid water = 4.184 J/g-K) a. 108 g b. 125 g c. 325 g d. 605 g e, 1.75 ×104 g 22.
0 0
Add a comment Improve this question Transcribed image text
Know the answer?
Add Answer to:
Ice at 0.0 °C is used to cool water. What is the minimum mass of ice...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for? Ask your own homework help question. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions
  • 2. 44.0 g of ice at –20.0 °C is mixed with 325 g of water at...

    2. 44.0 g of ice at –20.0 °C is mixed with 325 g of water at 32.1 °C. Calculate the final temperature of the mixture. Assume that no energy in the form of heat is transferred to the environment. (Heat of fusion = 333 J/g; specific heat capacities: ice = 2.06 J/g-K, liquid water = 4.184 J/g-K) ***HINT: Remember that ice melts at 0 °C***

  • z.hopts) How much energy(in kJ) must be removed from 71.8g of liquid water at 25.7°C to...

    z.hopts) How much energy(in kJ) must be removed from 71.8g of liquid water at 25.7°C to ice at -16.1°C? Given: Heat of fusion of water = 333J/g 71081 25.7--161 Ice specific heat capacity = 2.06 J/gK water specific heat capacity = 4.184 J/gK

  • An ice cube with a mass of 46.4 g at 0.0 ∘C is added to a...

    An ice cube with a mass of 46.4 g at 0.0 ∘C is added to a glass containing 4.20×102 g of water at 45.0 ∘C . Determine the final temperature of the system at equilibrium. The specific heat capacity of water, ?s , is 4.184 J/g⋅∘C , and the standard enthalpy of fusion, Δ?∘fus , of water is 6.01×103 J/mol . Assume that no energy is transferred to or from the surroundings.

  • An ice cube with a mass of 53.0 g at 0.0 °C is added to a...

    An ice cube with a mass of 53.0 g at 0.0 °C is added to a glass containing 368 g of water at 45.0 °C. Determine the final temperature of the system at equilibrium. The specific heat capacity of water, Cs, is 4.184 J/g·°C and the standard enthalpy of fusion, ΔH°fus, of water is 6.01 × 103 J/mol. Assume that no energy is transferred to or from the surroundings.

  • The temperature of 2.26 kg of water is 34 °C. To cool the water, ice at...

    The temperature of 2.26 kg of water is 34 °C. To cool the water, ice at 0 °C is added to it. The desired final temperature of the water is 11 °C. The latent heat of fusion for water is 33.5 × 104 J/kg, and the specific heat capacity of water is 4186 J/(kg·C°). Ignoring the container and any heat lost or gained to or from the surroundings, determine how much mass m of ice should be added.

  • What is the final temperature, (in oC), after a 26.5 gram piece of ice at 0oC...

    What is the final temperature, (in oC), after a 26.5 gram piece of ice at 0oC is placed into a styrofoam cup with 117.0 grams of water initially at 76.5oC? Assume no loss or gain of heat from the surroundings. Enter your answer without units. heat of fusion of water is 333 J/g. The specific heat of H2O(l) is approximately constant at 4.184 J/gK.

  • 3 pts Question 11 A 126 gram sample of ice was heated from 11.4°C to 42°C....

    3 pts Question 11 A 126 gram sample of ice was heated from 11.4°C to 42°C. The Specific Heat of ice = 2.09 J/gºC; Specific Heat of water = 4.184 J/gºC; and the Heat of fusion of ice = 334 J/g. Calculate the heat required to form liquid H2O up to 42°C. 221x104) 1.11 x 104) -2.21 x 104) -1.11 x 104)

  • You add 100.0 g of water at 51.0 °C to 100.0 g of ice at 0.00...

    You add 100.0 g of water at 51.0 °C to 100.0 g of ice at 0.00 °C. Some of the ice melts and cools the water to 0.00 °C. When the ice and water mixture reaches thermal equilibrium at 0 °C, how much ice has melted? (The specific heat capacity of liquid water is 4.184 J/g · K. The enthalpy of fusion of ice at 0 °C is 333 J/g.) Mass of ice = References Use the References to access...

  • An 12 g ice cube at -19?C is put into a Thermos flask containing 100 cm3...

    An 12 g ice cube at -19?C is put into a Thermos flask containing 100 cm3 of water at 20?C. By how much has the entropy of the cube-water system changed when a final equilibrium state is reached? The specific heat of ice is 2200 J/kg K and that of liquid water is 4187 J/kg K. The heat of fusion of water is 333 × 103 J/kg. An 12 g ice cube at -19 C is put into a Thermos...

  • 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 24.1 g of steam at 158°C is condensed, cooled, and frozen to ice at -50.°C.

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT