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.
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.
It freezes.
decreases
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.
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 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 to a liquid
Q=m s dT m = s dT/Q = 0.00924 X (100-25.3)/125 = 0.0055122 g
You remove heat. Nitrogen must be cooled to -196 degrees Celsius to become a liquid.
-273 degrees Celsius is nearly 0 Kelvin or absolute zero. While it is believed that it is impossible to achieve a temperature of absolute zero, all gases will solidify before that happens. A pure gas should form perfect crystals.
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.
If fifty grams of water cooled from 50 degrees to 10 degrees, and the specific heat of water is 4.2, 135 kJ of heat was released.
Question makes no sense - unanswerable. Nothing changes mass when heated or cooled.