Question

How much ice at 0◦C must be mixed with 60.0 g of water at 85.0 ◦C to give a final water temperature of 10◦C?

Answer #1

(a) How much ice at -14.2 C must be placed in 0.150 kg of water
at 18.4 C to cool the water to 0.0 C and melt all of the ice?
___0.0318__ kg
(b) If half that amount of ice is placed in the water, what is
the final temperature of the water?
____????___ degrees Celcius

when 50 g of ice at 0 degree c is placed in 400 g of water at 55
degree c, the final temperature is 40 degree c. if we ignore any
exchange of heat to the surroundings, how much heat does it take to
melt 1 g of ice at 0 degree c

Steam initially at 100° C is mixed with 150 g of ice at -60.0°
C, in a thermally insulated container. When the system comes to
thermal equilibrium, everything inside the container has been
converted into liquid water at 50° C. What is the entropy change of
the steam during the process? please show each step.

How much heat would it take to convert 60.0 g ice at 0.00˚C into
liquid water at 20.0˚C?
The trend in polarizability from left to right across a period
in the Periodic Table is due to …
a.
decreasing electronegativity.
b.
decreasing ionization energy.
c.
increasing mass.
d.
decreasing atomic size.

How much ice (in grams) must melt to lower the temperature of
351 mL of water from 26 ∘C to 4 ∘C ? (Assume the density of water
is 1.0 g/mL and that the ice is at 0 ∘C, the heat of fusion of ice
is 6.02 kJ/mol.)

If 20 g of ice at 0 °C is added to 180 g of water at 22 °C, what
will the final temperature of the water be?

A 50.0-g copper calorimeter contains 210 g of water at 20.0°C.
How much steam at 100°C must be condensed into the water if the
final temperature of the system is to reach 60.0°C?
A step-by-step process (ex. Q1+Q2+...+ Qn = 0) would be
appreciated. I am not concerned with the answer; I would just like
a clear setup of the problem.

1.) How much cold water at 4.26 degree C must be added to 667 g
of water at 45 degree C such that the final temperature of the
mixture is 25.0 degree C? No heat is exchanged with the
surroundings. Express your answer in grams.
2.) Calculate the amount of heat, in kJ, required to turn 511 g
of ice at -15.30C into water at 250C.

How much energy in kilojoules is needed to melt 60.0 g of ice
starting at −35.0∘C? (The specific heat of ice is 2.09Jg∘C and the
enthalpy of fusion is 6.01kJmole).

A 40-g block of ice is cooled to −70°C and is then added to 570
g of water in an 80-g copper calorimeter at a temperature of 22°C.
Determine the final temperature of the system consisting of the
ice, water, and calorimeter. (If not all the ice melts, determine
how much ice is left.) Remember that the ice must first warm to
0°C, melt, and then continue warming as water. (The specific heat
of ice is 0.500 cal/g · °C...

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