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No. When water is cooled it contracts up to 4 degrees Celsius and then it begins to expand till 0 degrees Celsius. This is called the anomalous expansion of water.
water True, but only in the range 4 degrees Celsius to zero Celsius.
It has to be cooled to below -196 degrees Celsius or -321 degrees Fahrenheit.
Q=m s dT m = s dT/Q = 0.00924 X (100-25.3)/125 = 0.0055122 g
It depends on it's original temperature and how much it was heated.
It will gradually drop to below 10 degrees.
Sort of. In the temperature range of 0-4 Degrees Celsius water contracts when heated and expands when cooled. Outside of this temperature range it behaves normally.
Cooled temperatures are still temperatures!. You can measure them using expansion thermometers down to around -15 deg Celsius. Below that you will probably need a thermocouple.
It would be -221.7 deg C.
Polythene takes its temperature from its surrounds, as do all substances unless specifically heated or cooled.
Hydrogen, helium, nitrogen, oxygen, fluorine, neon, chlorine, argon, bromine, krypton, xenon and radon are all gases at 100 deg C. Only Bromine will condense if cooled to room temperature.
No. When water is cooled it contracts up to 4 degrees Celsius and then it begins to expand till 0 degrees Celsius. This is called the anomalous expansion of water.
It does except when the temperature is close to 4 Celsius degrees. At this temperature water actually expends a little bit. But when you move further from 4 degrees towards negative temperatures it starts to shrink again as does when it comes from higher temperatures to 4 Celsius.
The same as most substances, CO2 must be cooled and put under increased pressure to become a solid. At one atmosphere, CO2 must be cooled to a temperature of -78.5 degrees Celsius to solidify. At height pressures CO2 solidifies at higher temperatures, however solid CO2 never exists at a temperature above -56.4 degrees Celsius.
Assuming the amount of gas remains constant, we can use the ideal gas law to calculate the final absolute pressure. The initial pressure (P1) is 200 kPa and the final volume (V2) is 250 cm3. The initial temperature (T1) is 40 degrees Celsius or 313.15 Kelvin, and the final temperature (T2) is 20 degrees Celsius or 293.15 Kelvin. Using the equation (P1 * V1) / T1 = (P2 * V2) / T2, we can solve for the final absolute pressure (P2), which is approximately 400 kPa.
When liquid water is cooled, it contracts like one would expect until a temperature of approximately 4 degrees Celsius is reached. After that, it expands slightly until it reaches the freezing point, and then when it freezes it expands by approximately 9%
increases