Question

Consider two 35-gram ice cubes, each initially at -5°C. One is
dropped into a at container filled with 0.1 kg of liquid nitrogen
(initially the boiling point of nitrogen); the other cube is
dropped into a container filled with 1 kg of (liquid) water,
initially at 5°C. Assume that no heat is lost through either
container (or into the atmosphere)

a) Describe what happens to each ice cube (and why)

b) If (Lv)Nitrogen =48 kcal/kg, (LF)Nitrogen = 6.1 kcal/kg,
and cNitrogen =0.15 kcal/(kg °C), determine how much heat would be
needed to produce 100 grams of nitrogen gas at 20°C.

c).Determine the final (equilibrium) temperature of the
icewater mixture.

d) Determine the phase (ie., liquid or solid) corresponding to
the equilibrium temperature you obtained in part (c).

Answer #1

a) Boiling point of nitrogen is -195.8 C, and the ice cube is at
-5 C, so the ice cube's temperature drops to further lower level
and there is no change of state pf the ice cube when put in boiling
noitrogen

Water is at 5 C, ice cubes are at -5C so the ice cubes start to
melt when put in water

b) heat = Lv*m + mcdT = 48*0.100 + 0.15*0.1*(20-(-195.8)) = 8.037
kCal

c) initial temperature of water, tw = 5 C

final temperature = T

initial mass of water, m = 1 kg

initaial temperature of ice = -5C = ti

initial mass of ice . M = 0.035 kg

hence from heat conservation'

energy lost by ice energy gained by water

MLf * Mc(ti) + MC(T - ti) = mC(tw - T)

here, Lf is latent heat of fusion of water, c is heat capacity of
ice, C is heat capacity of water

0.035(333550 + 2108*5 + 4187(T + 5)) = 1*4187(5 - T)

T = 1.8827 C

d) Final phase = liquid

Consider two 35-gram ice cubes, each initially at -5°C. One is
dropped into a at container filled with 0.1 kg of liquid nitrogen
(initially the boiling point of nitrogen); the other cube is
dropped into a container filled with 1 kg of (liquid) water,
initially at 5°C. Assume that no heat is lost through either
container (or into the atmosphere)
a) Describe what happens to each ice cube (and why)
b) If (Lv)Nitrogen =48 kcal/kg, (LF)Nitrogen = 6.1 kcal/kg,
and...

Consider two 35-gram ice cubes, each initially at -5°C. One is
dropped into a at container filled with 0.1 kg of liquid nitrogen
(initially the boiling point of nitrogen); the other cube is
dropped into a container filled with 1 kg of (liquid) water,
initially at 5°C. Assume that no heat is lost through either
container (or into the atmosphere).
1.Determine the final (equilibrium) temperature of the
icewater mixture.
2. Determine the phase (ie., liquid or solid) corresponding to
the...

A 35.0-g cube of ice, initially at 0.0°C, is dropped into 180.0
g of water in an 70.0-g aluminum container, both initially at
35.0°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.)
26.4 °C
17.6 °C
8.79 °C
35.1 °C
30.8 ° C

Two 50 gram ice cubes are dropped into 200 grams of water in a
class. 1.) if the water was initially at a temperature of 25
degrees C, and if the ice came directly from a freezer operating at
-15 degrees C, what will be the final temperature of the drink? The
specific heat of ice is about 0.50 cal/(gram degree C) in this
temperature range, and the heat required to melt ice to water is
about 80 cal/gram. 2.)...

(a) Two 64 g ice cubes are dropped into 278 g of water in a
thermally insulated container. If the water is initially at 25°C,
and the ice comes directly from a freezer at −15°C, what is the
final temperature at thermal equilibrium? (in celcius)
(b) What is the final temperature if only one ice cube is used?
(in celcius)

Three 100. g ice cubes are dropped in 750. grams of water (at
70.00 C) in a Styrofoam cup.
If the ice cubes were initially at -150C, how much
energy is necessary to warm and melt the ice cubes?
Will the ice cubes
melt?
Cice = 0.53
cal/g*OC
Lf = 79.5 cal/g
What is the final temperature of the system?

(a) You took two 49-gram ice cubes from your -14C kitchen
freezer and placed them in 201 g of water in a thermally insulated
container. If the water is initially at 24C, what is the final
temperature at thermal equilibrium? (b) What is the final
temperature if only one ice cube is used? Hint: Watch out for the
different possibilities!

Three 102.0-g ice cubes initially at 0°C are added to 0.810 kg
of water initially at 18.0°C in an insulated container.
(a) What is the equilibrium temperature of the system?
(b) What is the mass of unmelted ice, if any, when the system is
at equilibrium?

A 39.2 g cube of ice, initially at 0.0 °C, is dropped into 220 g
of water in an 80-g aluminum container. The water is initially at
35 °C and the aluminum container is initially at 25 °C. Remember to
take in to account the melting of the ice. What is the final
equilibrium temperature in °C?

30. A 0.035-kg ice cube at -30.0 C is placed in 0.33 kg of 35.0
C water in a very well-insulated container. The latent heat of
fusion for water is Lf=79.8 kcal/kg.
What is the final temperature of the water, in degrees
Celsius?

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