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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.
It would be -221.7 deg C.
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.
q = (42.5 g)(0.902 J/gC)(25o C - 4750o C) = - 1.8 X 105 Joules ====================negative can be ignored for absolute value, but remember the direction the heat is going.
It freezes.
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.
The pressure inside the container would decrease.
increases......
It has to be cooled to below -196 degrees Celsius or -321 degrees Fahrenheit.
It will gradually drop to below 10 degrees.
water True, but only in the range 4 degrees Celsius to zero Celsius.
32 g KCl
Gas pressure decreases when cooling down a closed container.
No. Car engines are cooled by water (under pressure), so they run at or aground 100 degrees Celsius. Of cause in the combustion chamber and at the exhaust temperatures are much higher.
gas to a liquid
Formula:P1 P2---- = ----T1 T2P1= 740 mm HgP2= UnknownT1= 22°C= 295 KT2= -22°C= 251 K740 / 295 = P2 / 251P2= 630 mm Hg
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.