judy places 0.150kg of boiling water at 100° C in a
thermos bottle. how many kilograms...
judy places 0.150kg of boiling water at 100° C in a
thermos bottle. how many kilograms of ice at -12.0°C must judy add
to the thermos so that the equilibrium temperature of the water is
75.0°C?
A. The boiling point of water is
100.0°C at 1 atmosphere.
How many grams of chromium(II) chloride
(122.9 g/mol), must be dissolved in
256.0 grams of water to raise the
boiling point by 0.300°C? Refer to the table for
the necessary boiling or freezing point constant.
Solvent
Formula
Kb (°C/m)
Kf (°C/m)
Water
H2O
0.512
1.86
Ethanol
CH3CH2OH
1.22
1.99
Chloroform
CHCl3
3.67
Benzene
C6H6
2.53
5.12
Diethyl
ether
CH3CH2OCH2CH3
2.02
____g chromium(II) chloride.
B. The boiling point of water...
A pot with boiling water at 100 C, if the handle is 3 mm thick,
22 mm wide, 300 mm long and exposed tp 19 C temp, h= 5 w/m2 c.
What is the temp at the end of the handle if it is k= 13, and
then if it was k = 180 W/m.k
What kind of assumptions
Does insulation need to be on the intire handle from being
burned why?
A bottle of Dasani water has a volume of 500 milliliters. How
many moles of water are in the bottle? Give your answer to three
significant figures.
2. How many iron atoms are in a 6.75 lb iron railroad spike?
3. What is the mass of 0.0023 moles of NaCl? Give your answer in
milligrams.
For ochem
Rank the boiling point of water at these following three places.
Explain why?
A) Deat Valley, Elevation -285 ft, P=1.01 atm
B) New York City, Elevation 0 ft, P=1.00 atm
c) Laramie, WY, Elevation 7165 ft, P=0.75 atm
In column chromatography. what would happen if the elution
solvent is too polar?
How many kilograms of water can be evaporated from a 1
m^2 surface in a lake on a hot summer day, if it is assumed that
the limiting factor is solar insolation (1000 W/m^22). Assume that
the length of the day is 8 hours and that the air and water temp
are at 40 degrees Celsius. B. What volume of air is needed to hold
this much water vapor at 40 oC. C. When the sun sets, the air
temperature...
An insulated Thermos contains 145 g of water at 70.7 ˚C. You put
in a 11.0 g ice cube at 0.00 ˚C to form a system of ice + original
water. The specific heat of liquid water is 4190 J/kg•K; and the
heat of fusion of water is 333 kJ/kg. What is the net entropy
change of the system from then until the system reaches the final
(equilibrium) temperature?
An insulated Thermos contains 128 g of water at 81.3 ˚C. You put
in a 12.5 g ice cube at 0.00 ˚C to form a system of ice +
original water. The specific heat of liquid water is 4190
J/kg•K; and the heat of fusion of water is 333 kJ/kg. What is the
net entropy change of the system from then until the system reaches
the final (equilibrium) temperature?