100 g of ice at -20°C are mixed with 250 g of water at 20°C in
an insulated calorimeter. What is the final temperature of the
system? How many grams of liquid water and how many grams of ice
will you find after the system equilibrates? find T in degrees C; m
of solid (in grams); m of liquid (in grams)
T=____
ms=____
mliq=____
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.
A) Find the final temperature of the system, assuming no heat
losses. (Assume that the specific heat of ice is 2.0 kJ/kg K)
B) A second 200 g piece of ice at -20 C is added. How much ice
remains in the system after it reaches equilibrium?
C) Would your answer...
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 to part b...
20 liters of water at 20 bar and 100 °C are in a variable volume
container. 56,000 kJ of heat are added to the system at constant
pressure which causes an increase in both temperature and
volume.
Draw a schematic of the process
Write the energy balance for this process and clearly state any
assumptions:
What is the final volume of the container?
How much work in [kJ] is completed? Pay careful attention to
your negative signs!
In one sentence...
A water sample obtained from the neigborhood pond was analyzed
for dissolved oxygen content. A volume of 300 mL, with temperature
21 degrees Celsius, was analyzed using the Wrinkler method shown in
the simulated lab material. It took 15.0 mL of 0.01 mol/L Na2S2O3
solution to reach titration end point.
*Note: Na2S2O3 solution is the source of S2O32- ions for the
titration reaction.
In the succeeding questions, provide the following values
required. Take note of the units
a.What is the...
(a) What is the total volume of gaseous products, measured at
350°C and 689 torr, when an automobile engine burns 103 g of C8H18
(a typical component of gasoline)? L (b) For part (a), the source
of O2 is air, which is about 78.0% N2, 21.0% O2, and 1.0% Ar by
volume. Assuming all the O2 reacts, but no N2 or Ar does, what is
the total volume of gaseous exhaust?
A 200 g aluminum calorimeter contains 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. (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 to part b be different if...
Consider a solution of 1.00 g of glucose in 100 g of water at
20˚C (where the vapor pressure of pure water is 17.54 torr). For
this problem we will assume the solution behaves ideally.
(a) What is the equilibrium vapor pressure of the
solution?
(b) What is the osmotic pressure of the solution versus pure
water (report it in torr)?
(c) What is the activity of water as a solvent in the
solution?
(d) Now suppose 1.00 g of...