[References) When ice at 0°C melts to liquid water at 0°C, it absorbs 0.334 kJ of heat per gram. Suppose the heat needed to
melt 40.5 g of ice is absorbed from the water contained in a glass. If this water has a mass of 0.223 kg and a
temperature of 21.0°C, what is the final temperature of the water? Assume the specific heat is that of pure water,
4.18 J/(g•°C). (Note that you will also have 40.5 g of water at 0°C from the ice.)
Temperature =
°C
Submit Answer
Try Another Version
9 item attempts remaining

the answer

explanation:

the capillary tube was too close to the bottom of the beaker.

the ruler may have moved.

water got into the capillary tube.

the temperature was not allowed to equilibrate in the 2-4 minutes.

hey there!

boiling point is the temperature at which the vapor pressure of the liquid equals atmospheric pressure. the vapor pressure of solvent molecules is decreased when a solute is added, so a higher temperature is required to increase the number of solvent molecules in the gas phase above the liquid.

at the freezing point, the vapor pressures of the solid and liquid are equal; a lower temperature is needed to reduce the number of solvent particles above the liquid.

hope this you

tobey