In the previous question you were provided with an extra piece of information: You were told that only liquid water would be present once equilibrium was established. If the final state of a system is not given, it is still possible to determine it from the initial temperatures and masses. The next few parts will help illustrate this point. Suppose that in an insulated container, 0.100 kg of water at 20.0∘C is mixed with 1.500kg of ice at −15.0∘C. You are asked to find the final temperature Tf of the system, but you are not told what the final phase of the system in equilibrium is.
Part F:Find the amount of heat Qh it would take to bring all
of the ice to its melting point, 0∘C. ANSWER IS Qh =
4.70×104 J
Part G: Find the amount of heat Qc released in bringing all of the
water to its freezing point, 0∘C. Your answer does not need to
include a sign.
ANSWERS IS: Qc = 8380 J
Part H: Question:
Suppose the water is at its freezing point, 0∘C, but has not yet
turned to ice. Find the amount of heat Qf released during the
water's phase transition to ice. Your answer does not need to
include a sign
In the previous question you were provided with an extra piece of information: You were told...
In the previous question you were provided with an extra piece of information: You were told that only liquid water would be present once equilibrium was established. If the final state of a system is not given, it is still possible to determine it from the initial temperatures and masses. The next few parts will help illustrate this point. Suppose that in an insulated container, 0.100 kg of water at 20.0∘C is mixed with 1.500kg of ice at −15.0∘C. You...
I need help with Number 5, Thank you! 5. Suppose 150g of ice at a temperature of 0 C are combined with 250 g of water at 70°C.in tainer. The onty heat nges are between the ice and the water. You have been asked to predict the final state of the system. Consult the appropriate tables in b the text for any numbers you need a) One possible outcome is that the system might cool down to O'C, resulting in...
Prob. 2: Cooling Curve Circle: Emathermier Exothermis?) Cale, the amount of heat this time in calories (cal) - Ilse I cal 4184 for conversions) lost or removed From 1.75 mol water as steam at a convert it to solid ice chilled in a freezer to a temperature of 47.2°C Cumulative Heat Lost To do this, follow the above drawn curve to determine the amount of heat lost for each of the five steps of this process to convert superheated steam...
Can you show all work and calculations. Thank you so much!! 3. In an insulated vessel, 500 g of ice at-5°C is added to 250 g of water at 50.0℃ (a) What is the final temperature of the system? (b) How much ice remains when the system reaches equilibrium? Specific heat for water and ice are C,-4186 J/kg °C) and Cie-2108 J/(kg·C), respectively, and latent heat of fusion for water is Lf- 3.33 x 105 J/kg NOTES - If all...
please answer all questions Temperature Change and Heat Capacity - Calorimetry- Two substances The quantitative relationship between heat transfer and temperature change is Q = mcAT, where Q is heat transfer, m is the mass of the substance, and AT is the change in temperature. The symbol c stands for specific heat and depends on the material and phase. The specific heat c is the amount of heat necessary to change the temperature of 1.00 kg of mass by 1.00°C....
(20%) Problem 2: A piece of unknown material has a mass of m, = 0.79 kg and an initial temperature of Tu = 79°C. The specific heat of water is cw = 4.180 x 102 J/(kg:°C). 50% Part (a) The sample of material is dropped into my = 1.4 kg of water at T = 19°C in a calorimeter. The calorimeter reaches a final temperature of Te = 34°C. Enter an expression for the specific heat of the unknown material,...
A 210 g piece of ice at 0°C is placed in 480 g of water at 25°C. The system is in a container of negligible heat capacity and is insulated from its surroundings. (a) What is the final equilibrium temperature of the system? °C (b) How much of the ice melts? g
(10%) Problem 4: You are on your way to a party when the host asks you to pick up a bag of ice. At the grocery store you grab a 7. kg bag that was kept at a temperature of -3.7 C. When you get to the party, you find a large cooler to put the ice in. There is already 28 L (ie., 28 kg) of water in the cooler at a temperature of 21°C. You toss the ice...
A) A 41 g ice cube at −21◦C is dropped into a container of water at 0◦ C. How much water freezes onto the ice? The specific heat of ice is 0.5 cal/g ·◦ C and its heat of fusion of is 80 cal/g. Answer in units of g. B) A 0.0602 kg ingot of metal is heated to 205◦C and then is dropped into a beaker containing 0.411 kg of water initially at 18◦C. If the final equilibrium state...
Calculate the final equilibrium temperature when 10.0 grams of steam initially at 100 degree C is mixed with 450 grams of liquid water and 110 grams of ice at 0 degree C in a calorimeter. That is, the liquid water AND the ice are initially at 0 degree C. Ignore any heat energy exchanges with the calorimeter and the surroundings. If you conclude that the final temperature of the system is 0 degree C, then what mass of ice remains,...