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.

Expert Solution

genius_generous answered 2 years ago

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.

Steam at 100°C is condensed into a 54.0 g aluminum calorimeter cup containing 260 g of...

Steam at 100°C is condensed into a 54.0 g aluminum calorimeter cup containing 260 g of water at 25.0°C. Determine the amount of steam (in g) needed for the system to reach a final temperature of 64.0°C. The specific heat of aluminum is 900 J/(kg · °C).

A 200 g insulated aluminum cup at 16 ∘C is filled with 255 g of water...

A 200 g insulated aluminum cup at 16 ∘C is filled with 255 g of water at 100 ∘C a) Determine the final temperature of the mixture. b) Determine the total change in entropy as a result of the mixing process (use ΔS=∫dQ/T).

A 50·g ice cube (at 0°C) is placed in an insulated cup with 250·g of water...

A 50·g ice cube (at 0°C) is placed in an insulated cup with 250·g of water which is at 46°C. The latent heat of fusion for ice is 80·cal/g and the specific heat of water is 1.0·cal/g/°C. (a) How much heat will the ice have to absorb from the water to completely melt (and turn into 0°C water)? ___ cal. (b) Find the temperature of the 250·g of water initially at 46°C after it loses the heat required to melt...

Part A The aluminum cup inside your calorimeter weighs 42.95 g. You add 60.51 g of...

Part A The aluminum cup inside your calorimeter weighs 42.95 g. You add 60.51 g of 1.0 M acetic acid solution and 49.33 g of 1.0 M sodium hydroxide solution to the calorimeter. Both solutions have an initial temperature of 19.9 oC, and the final temperature after addition is 26.7 oC. What is the heat of neutralization for the amounts of reactants used, in units of J? Assume that: the calorimeter is completely insulated the heat capacity of the empty...

When 28 g of calcium chloride was dissolved in 100g water in a coffee-cup calorimeter, the...

When 28 g of calcium chloride was dissolved in 100g water in a coffee-cup calorimeter, the temperature rose from 25* Celcius to 41.3. What is the enthalpy change for this process? Assume the solution is equal to the specific heat of water.

An insulated container contains 15.0 g of steam at 100C. A mass of 65.0 g of...

An insulated container contains 15.0 g of steam at 100C. A mass of 65.0 g of ice at 0.00C is dropped into the container (assume no energy is absorbed by the container). C = Celsius a). How much heat is released by the steam when it condenses at 100C? (Qs) b). How much heat is absorbed by the ice when it melts at 0.00C? (Qi) c). What is the final temperature of the the water in the container? (T)

A 26.0-g aluminum block is warmed to 65.1 ∘C and plunged into an insulated beaker containing...

A 26.0-g aluminum block is warmed to 65.1 ∘C and plunged into an insulated beaker containing 55.5 g of water initially at 22.3 ∘C . The aluminum and the water are allowed to come to thermal equilibrium. (Cs,H2O=4.18J/g⋅∘C , Cs,Al=0.903J/g⋅∘C ) Assuming that no heat is lost, what is the final temperature of the water and aluminum? T = ?? ∘C

A 25 g piece of hot iron is dropped into a glass of ice water containing...

A 25 g piece of hot iron is dropped into a glass of ice water containing 15.0 g of ice and 50.0 g of water. If the iron loses 8.00 kJ of energy to the ice water in achieving equilibrium, what is the equilibrium temperature? ∆Hfus = 6.01 kJ/mol

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...

Question