Question

If you have 0.381 m^{3} of water at 25.0 ∘C and add
0.142 m^{3} of water at 95.0 ∘C , what is the final
temperature of the mixture? Use 1000 kg/m^{3} as the
density of water at any temperature.

Final temperature =?

Answer #1

If you have 410.0 g of water at 25.00 °C in an insulated vessel
and add 120.0 g of water at 95.00 °C, what is the final temperature
of the mixture?

1.00 kg of ice at -38.0 degrees C is dropped into 25.0 kg of
water at 34.0 degrees C. What is the final temperature of the
mixture?

A 25.0-g glass tumbler contains 200 mL of water at 24.0ºC. If
two 15.0-g ice cubes, each at a temperature of –3.00ºC, are dropped
into the tumbler, what is the final temperature of the drink?
Neglect any heat transfer between the tumbler and the room.
(Specific heat of water and ice are 4.186 kJ/(kg K) and 2.05 kJ/(kg
K), respectively. The latent heat of fusion of water is 333.5
kJ/kg. The specific heat of glass is 0.840 kJ/(kg K )....

The density of water at 0°C is very nearly 1000 kg/m3
(it is actually 999.84 kg/m3), whereas the density of
ice at 0°C is 917 kg/m3. The bulk modulus of ice is 2.20
× 109 Pa. Calculate the pressure,
in pascals, necessary to keep freezing water from expanding,
neglecting the effect such a large pressure would have on the
freezing point. (This problem gives you only an indication of how
large the forces associated with freezing water might
be.)

(a) An insulated container holds 2.0 kg of water at 303 K. You
add 0.15 kg of ice at 273 K. When the mixture comes to equilibrium,
what is its final temperature?
cwater = 4186 J/kg K
Lfusion ice/water = 3.34 x 105 J/kg
(b) An insulated container holds 2.0 kg of water at 303 K. You
add a piece of copper with mass 0.10 kg. The combination comes to a
final temperature of 307 K. What was the original...

If you combine 360.0 mL of water at 25.00 °C and 130.0 mL of
water at 95.00 °C, what is the final temperature of the mixture?
Use 1.00 g/mL as the density of water.

If you combine 330.0 mL of water at 25.00 °C and 130.0 mL of
water at 95.00 °C, what is the final temperature of the mixture?
Use 1.00 g/mL as the density of water.

If you combine 440.0 mL of water at 25.00 °C and 140.0 mL of
water at 95.00 °C, what is the final temperature of the mixture?
Use 1.00 g/mL as the density of water.

If you combine 430.0 mL of water at 25.00 °C and 130.0 mL of
water at 95.00 °C, what is the final temperature of the mixture?
Use 1.00 g/mL as the density of water.

If you combine 280.0 mL of water at 25.00 °C and 140.0 mL of
water at 95.00 °C, what is the final temperature of the mixture?
Use 1.00 g/mL as the density of water.
Answer: _____celsius

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