A 9.0×10−2-kg ice cube at 0.0 ∘C is dropped into a Styrofoam cup holding 0.35 kg...

A 9.0×10⁻²-kg ice cube at 0.0 ∘C is dropped into a Styrofoam cup holding 0.35 kg of water at 11 ∘C.

Find the final temperature of the system. Assume the cup and the surroundings can be ignored.

Find the amount of ice (if any) remaining.

Find the initial temperature of the water that would be enough to just barely melt all of the ice.

Express your answer using two significant figures.

Expert Solution

genius_generous answered 2 years ago

An ice cube of mass 0.029 kg and temperature -13 ∘C is dropped into a styrofoam...

An ice cube of mass 0.029 kg and temperature -13 ∘C is dropped into a styrofoam cup containing water of mass 0.4 kg and temperature 20 ∘C. Calculate the final temperature in degrees celcius and give your answer to one decimal place. (For simplicity, we ignore here the temperature change of the cup.) The specific heat of ice is 2200 J/kg ∘C and the specific heat of water is 4186 J/kg ∘C. The latent heat of fusion of ice is...

A 50-g cube of ice, initially at 0.0°C, is dropped into 200 g of water in...

A 50-g cube of ice, initially at 0.0°C, is dropped into 200 g of water in an 80-g aluminum container, both initially at 30°C. What is the final equilibrium temperature? (Specific heat for aluminum is 900 J/kg×°C, the specific heat of water is 4 186 J/kg×°C, and Lf = 3.33 ´ 105 J/kg.)

A 116-g cube of ice at 0 ∘∘C is dropped into 1.26 kg of water that...

A 116-g cube of ice at 0 ∘∘C is dropped into 1.26 kg of water that was originally 84.1∘C. What is the final temperature of the water after the ice melts and the water comes to thermal equilibrium? This problem requires a lot of algebra. You will make fewer errors if you solve for the answer using symbols and then plug in the numbers. The specific heat of water and the latent heat of fusion for water are given in...

40.0 gram of ice at −15.00 °C is put into a Styrofoam cup calorimeter (of negligible...

40.0 gram of ice at −15.00 °C is put into a Styrofoam cup calorimeter (of negligible mass) containing water at +15.00 °C. When equilibrium is reached, the final temperature is 6.00 °C. How much water did the calorimeter contain initially? The specific heat of ice is 2090J/(kg • K), that of water is 4186 J/(kg • K), and the latent heat of fusion of water is 33.5 × 104J/kg. A)416 g B)579 g C)425 g D)613 g E)780 g

1. A 100 g ice cube at -10?C is placed in an aluminum cup whose initial...

1. A 100 g ice cube at -10?C is placed in an aluminum cup whose initial temperature is 70?C. The system comes to an equilibrium temperature of 20?C. What is the mass of the cup in kg. 2.Radiation from the head is a major source of heat loss from the human body. Model a head as a 20-cm-diameter, 20-cm-tall cylinder with a flat top.If the body's surface temperature is 36 ?C , what is the net rate of heat loss...

A 70.0 g ice cube at 0.0 degrees C is placed in a lake whose temperature...

A 70.0 g ice cube at 0.0 degrees C is placed in a lake whose temperature is 18.0 degrees C. Calculate the change in entropy (in joules/Kelvin) of the system as the ice cube comes to thermal equilibrium with the lake. (c for water = 4186 J/kg-K)

28 g of ice at -10⁰C is dropped in an insulated 75-g aluminum calorimeter cup containing...

28 g of ice at -10⁰C is dropped in an insulated 75-g aluminum calorimeter cup containing 140 g of water at 30⁰C. (a) Calculate the equilibrium temperature of the container. Specific heats of liquid water, ice and aluminum are 4186 J/(kg ⁰C), 2090 J/(kg ⁰C) and 910 J/(kg ⁰C)respectively. Latent heat of fusion for ice is 3.33 x 105 J/kg. (b) What if, find the final temperature if 68 g of ice had been dropped.

An 18.0 g ice cube initially at -10 Celsius is dropped into 120g of water initiallly...

An 18.0 g ice cube initially at -10 Celsius is dropped into 120g of water initiallly at 25 Celsius. What is the final temperature of the system after all of the ice has melted? Assume that no heat is lost to the container or the surroundings

1.45 kg of ice at -5 ∘C is dropped into 31 kg of water at temperature 15.3 ∘C . Part...

1.45 kg of ice at -5 ∘C is dropped into 31 kg of water at temperature 15.3 ∘C . Part A - Final Temperature What is the final temperature of the system? (If I've set the problem up right, you should be given numbers such that all of the ice has melted.) Tf = ∘C Part B - Entropy of Warming Ice What is the change in entropy of the ice, as it warms up before melting? S = J/K Part C - Entropy...

A 5-gram ice cube at -2 degrees Celsius is dropped into 60 grams of liquid water...

A 5-gram ice cube at -2 degrees Celsius is dropped into 60 grams of liquid water at 12 degrees Celsius. If the ice and water are isolated from the environment, what is the final temperature of the combined liquid water when all of the ice has melted and the mixture reaches thermal equilibrium?

Question