Question

A 0.033 kg glass (with c = 840 J/kg oC) contains 0.281 of lemonade which, due to the sugar content, has a specific heat of 4,208 J/kg oC. After putting 0.049 kg of ice into the glass and allowing it to completely melt the final equilibrium temperature of the glass of lemonade is found to be 2.9 oC. intial temperature is 0.

(a) Calculate the initial temperature of the lemonade and glass. oC

Note the following data for ice/water: specific heat (ice)= 2100 J/(kg*oC) , Latent heat of fusion = 3.33 x 105 J/kg , melting/freezing point = 0 oC, specific heat (water) = 4186 J/(kg*oC)

Answer #1

Let the initial temperature of lemonade and glass be T degree C

Heat lost by lemonade and glass is

Heat gained by ice is

Equating the heat lost to heat gained

Solving this gives the initial temperature of the lemonade and glass

8.33 kg of steam at temperature of 150 ∘C has 2.23×107 J of heat
removed from it. Determine the final temperature and phase of the
result once the heat has been removed if the heat is removed at
constant pressure during the gas phase.
For this problem, use the specific heat (at constant pressure)
for water as 1850 J/kg∘C , the latent heat of vaporization as
2.256×106 J/kg , the specific heat of liquid water as 4186 J/kg∘C ,
the...

You have a pitcher with 2.00 L of water at an initial
temperature of 12.0 oC and you wish to add ice to it to bring the
temperature down. If the ice starts at an initial temperature of T1
= -18.4 oC, calculate the mass of ice required to reach a final
state of all liquid water at 0.00 oC. *****Assume no heat is gained
or lost to the surroundings.*****
More information:
Melting point of water - 0.00 degrees celcius...

8.33 kg of steam at temperature of 150 ∘C has 2.23×107 J of heat
removed from it. Determine the final temperature and phase of the
result once the heat has been removed if the heat is removed at
constant pressure during the gas phase. For this problem, use the
specific heat (at constant pressure) for water as 1850 J/kg∘C , the
latent heat of vaporization as 2.256×106 J/kg , the specific heat
of liquid water as 4186 J/kg∘C , the...

A 60 kg block of ice begins at -60 degrees the specific heat of
ice is 2090 j/(kg)C. The latent heat of fusion of water is 3.3 x
10^5 and the latent heat of vaporization is 2.3 x 10^6 J/kg. How
much energy is required to heat the ice to 0 degrees Celcius
(melting point)?
How much energy is required to heat the ice from -50C to the
melting point and melt the ice?
How much energy is required to...

A 7kg glass bowl contains 16kg of punch at 25oC. Two
and a half kilograms of ice is added to the punch. The ice has an
initial temperature of -20oC. Assume no transfer of heat
to the external environment when equilibrium is reached, all the
ice has melted and the final temperature of the mixture is above
0oC. Determine this temperature?
Cglass = 840 J.kg-1.oC
Cice = 2000 J.kg-1.oC
Latent heat of fusion of water, Lw = 335,000 J/kg

A 2.5 kg metallic block with an initial temperature of 80°C is
placed in a styrofoam cup containing 0.1 kg of ice at -15°C.
Assuming that no heat escapes from the cup what is the final
temperature of the metallic block? The specific heat of the metal
is 480 J/kg ∙ K, specific heat of ice is 2090 J/kg ∙ K, the latent
heat of fusion of water is 3.33 × 105 J/kg, and the specific heat
of water is...

A 24 g block of ice is cooled to −63◦C. It is added
to 572 g of water in a 98 g copper calorimeter at a temperature of
30◦C.
Find the final temperature. The specific heat of copper is 387
J/kg ·◦C and of ice is 2090 J/kg ·◦C. The
latent heat of fusion of water is 3.33 × 105 J/kg and its specific
heat is 4186 J/kg·◦C.
Answer in units of ◦C.

A 31 g block of ice is cooled to −90◦C. It is added to 591 g of
water in an 65 g copper calorimeter at a temperature of 26◦C. Find
the final temperature. The specific heat of copper is 387 J/kg · ◦C
and of ice is 2090 J/kg · ◦C . The latent heat of fusion of water
is 3.33 × 105 J/kg and its specific heat is 4186 J/kg · ◦C . Answer
in units of ◦C.

An insulating cup contains water at 25 ∘C. 30 grams of ice at 0
∘C is placed in the water. The system comes to equilibrium with a
final temperature of 14∘C. How much water in grams was in the cup
before the ice was added? (specific heat of ice is 2090 J/(kg
LaTeX: ^\circ∘C), specific heat of water is 4186 J/(kg LaTeX:
^\circ∘C), latent heat of the ice to water transition is 3.33 x10^5
J/kg)

How many joules heat must be added to 2.0 kg of ice at a
temperature of -30 °C to bring it to room temperature 20 °C?
(Specific heat capacity of ice is 2100 J/kg °C).
(Specific heat capacity of water is 4186 J/kg °C).
(Latent heat of water-ice is 3.33x105 J/kg)
Group of answer choices
126.52 kJ
959.44 kJ
4293.44 kJ
668.78 kJ

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 19 minutes ago

asked 19 minutes ago

asked 20 minutes ago

asked 23 minutes ago

asked 30 minutes ago

asked 30 minutes ago

asked 36 minutes ago

asked 59 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago