Question

Q4 A ZZ kg block of ice at -15 °C is added to an insulated container partially filled with 12 kg of water at 20 °C.

(Where ZZ = random number as shown in the attachment file. Note that if you do not use the proper numbers, your answer will be considered wrong.) Given: cw = 4186 J/kg.°C; cice = 2220 J/kg.°C, Lf = 3.34×10 5 J/kg

(a) Determine the final state of the mixture.

Explain your answer.

(b) Based on your answer in (a),

calculate either one (1) of the following: - the mass of ice that melts. - the final temperature of the system. (1 mark)

(c) Based on your answer in Q4(b), the system is then heated to 110°C. Assuming all water vaporizes, calculate the total energy of the system. Given: Lv = 2.26×10 6 J/kg, csteam = 2.01×10 3 J/kg.°C

Answer #1

A 11 kg block of ice at -15 °C is added to an insulated
container partially filled with 12 kg of water at 20 °C.
Given: Cw = 4186 J/kg. °C; Cice = 2220 J/kg. °C, L= 3.34x10
J/kg
(a) Determine the final state of the mixture. Explain your
answer.
Based on your answer in (a),
calculate either one (1) of the following: the mass of ice that
melts. the final temperature of the system.
(c) Based on your answer...

A well-insulated styrofoam bucket contains 142 g of ice at 0 °C.
If 24 g of steam at 100 °C is injected into the bucket, what is the
final equilibrium temperature of the system?(cwater=4186 J/kg.°C,
Lf=3.35 × 105 J/kg, Lv=2.26 × 106 J/kg)

1. 6.00kg of ice at −5.00 oC is added to a cooler holding 20
liters[careful not 30 liters] of water at 20.0 oC. What is the
final temperature? (neglect the heat capacity of the cooler.) (cw =
4186 J kg oC ; ci = 2010 J kg oC ; Lf = 3.33 × 105 ; Lv = 2.26 ×
106 ; ρw = 1.00g/cm

A well-insulated styrofoam bucket contains 146 g of ice at 0 °C.
If 24 g of steam at 100 °C is injected into the bucket, what is the
final equilibrium temperature of the system?(cwater=4186 J/kg.°C,
Lf=3.35 × 105 J/kg, Lv=2.26 × 106 J/kg). Answer in Degrees C.
Please provide a detailed answer. Thank you!

15 grams of ice at -5° C are brought into thermal contact with 6
grams of steam at 100° C.
If you have Cice = 2090 J/Kg°K , Cwater =
4186 J/Kg°C , Lf = 3.33x105 J/Kg and Lv =
2.26x106 J/Kg
Calculate the entropy change when the system reaches thermal
equilibrium

In a container of neglibible mass, a sample consiting of 0.180
kg of ice is at an initial termperature -40.0 degrees celsius. What
is the final temperature after 1.10 x 10^5 J of heat energy has
been added to the sample? For ice , c=2010 J/(kg*K) and for liquid
water c= 4190 J/ (kg*K). For water, Lf = 3.34 x 105 J/kg and Lv =
2.256 x 106 J/kg.

You have 1.60 kg of water at 27.0°C in an insulated container of
negligible mass. You add 0.640 kg of ice that is initially at
-22.6°C. Assume no heat is lost to the surroundings and the mixture
eventually reaches thermal equilibrium. If all of the ice has
melted, what is the final temperature (in °C, round to 2 decimal
places) of the water in the container? Otherwise if some ice
remains, what is the mass of ice (in kg, round...

You have 1.45 kg of water at 27.4°C in an insulated container of
negligible mass. You add 0.680 kg of ice that is initially at
-22.4°C. Assume no heat is lost to the surroundings and the mixture
eventually reaches thermal equilibrium. If all of the ice has
melted, what is the final temperature (in °C, round to 2
decimal places) of the water in the container? Otherwise
if some ice remains, what is the mass of ice (in kg, round...

How much heat is required to melt 2.0 kg of ice at 0°C?
[cice = 2108 J/kg·K; cwater = 4186 J/kg·K;
Lf = 3.33 x 105 J/kg; Lv = 22.6 x
105 J/kg]
Please write clearly and legibly!

A 0.66300.6630 kg ice cube at −12.40−12.40 °C is placed inside a
rigid, thermally isolated chamber containing steam at 365.0365.0
°C. Later, you notice that the ice cube has completely melted into
a puddle of water. The specific heats of ice, water, and steam are
?ice=2093 J/(kg·∘C),cice=2093 J/(kg·∘C), ?water=4186
J/(kg·∘C),cwater=4186 J/(kg·∘C), and ?steam=2009
J/(kg·∘C),csteam=2009 J/(kg·∘C), respectively.
If the chamber initially contained 6.1906.190 moles of steam
(water) molecules before the ice was added, calculate the final
temperature ?fTf of the puddle...

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