Question

question 1) answer clearly

In a calorimeter of negligible heat capacity, 200 g of steam at 150 ° C and 100 g of ice at -40 ° C are mixed. The pressure is maintained at 1 atm. What is the final temperature and how much steam, ice and water are present?

Answer #1

A 100-g piece of ice at 0.0oC is placed in an
insulated calorimeter of negligible heat capacity containing 100 g
of water at 100oC. (a) What is the final temperature of
the water once thermal equilibrium is established? (b) Find the
entropy change of the universe for this process.

A copper calorimeter can, having a heat capacity of 30 cal/deg,
contains 50 g of ice. The system is initially at 0oC. 12
g of steam at 100oC and 1 atm pressure are run into the
calorimeter. What is the final temperature of the calorimeter and
its contents?
Please show all work and be descriptive of what variable in the
equations are! Thank you :)

A well-insulated bucket of negligible heat capacity contains 134
g of ice at 0°C.
(a) If 21 g of steam at 100°C is injected into the bucket, what
is the final equilibrium temperature of the system?
°C
(b) What mass of ice remains?
g

Answer the following questions:
a) A calorimeter, specific heat capacity 500.0 J/kgC, mass 200.0
g, contains 300.0 g of water at 40.0 C. If 50.0 g of ice at 0.00 C
is dropped into the water and stirred, the temperature of the
mixture when the ice has melted is 23.8 C. Calculate the heat of
fusion of ice.
b) What is the final temperature attained when 900.0 g of ice at
0.00 C is dropped into 3400.0 g of water...

In a constant-pressure calorimeter of negligible heat capacity,
25 mL of 1.00 M CaCl2 is mixed with 25 mL of 2.00 M KF, resulting
in solid CaF2 precipitating out of the solution. During this
process, the temperature of the water rises from 25.0°C to 26.7°C.
Assume the specific heat capacity of the solution is 4.184 J/°C•g
and the density of the solution is 1.00 g/mL. Calculate the
enthalpy of precipitation in kJ per mole of CaF2 precipitated.

A 200 g aluminum calorimeter can contain 500 g of water at 20 C.
A 100 g piece of ice cooled to -20 C is placed in the
calorimeter.
- Find the final temperature of the system, assuming no heat
losses. (Assume that the specific heat of ice is 2.0 kJ/kg K)
- A second 200 g piece of ice at -20 C is added. How much ice
remains in the system after it reaches equilibrium?
- Would your answer...

A 102 g piece of ice at 0.0°C is placed in an insulated
calorimeter of negligible heat capacity containing 100 g of water
at 100°C. Find the entropy change of the universe for this
process?
135 J/K 134 J/K is wrong,

A nonconducting tank of negligible heat capacity and 1
m3
volume is connected to
pipeline containing steam at 5 bar and 370℃, filled with steam
to a pressure of 5 bar,
and disconnected from the pipeline. If the tank initially
contains steam at 1 bar and 150℃, how much steam is in the
tank at the end of the filling process, and what is its
temperature?
Note: The answer is 1.56kg and 425c but I can’t figure out how
to...

If 10 g of steam of 100 C is introducded into a mixture of 200 g
of water and 120 g of ice find the the final temperature and
composition of the mixture?
mass ice= 120g, c=0.5
mass water=200 g , c=1
Lf= 80 cal/ g Lv= 540 cal

Steam at 100°C is condensed into
a 38.0 g copper calorimeter cup containing 260 g of water at 27.0°C. Determine the amount of steam (in
g) needed for the system to reach a final temperature of
56.0°C. The specific heat of copper is
387 J/(kg
· °C).

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