This question can't be answered if you don't provide the chemical reaction's equation with this other data.
No, it does not. The volume of water changes according with it's temperature. Water, unlike other substances, it has a minimum volume at 4 degrees Celsius.
crystalline structures that tend to collapse when 0 degrees celsiurs in increased. The melting of these crystals further decreases the volume of the water. The water undergoes two processes at the same time- contraction and expansion. Volume tends to decrease as ice crystals collapse, while volume tends to increase due to great molecular motion
1,400 mL
It's most dense at 4 degrees celsius. Get any lower and it takes up more volume. As a general rule, chemicals get denser as they get colder.
Under very specific conditions - yes, but normally no. Except in a narrow range from about 0° to about 8 °C, a sample of water can only have the same volume after being warmed by several degrees Celsius if it is confined in a fixed volume container. Liquid water is slightly compressible so if you place it inside a container where it can be compressed, you can heat it a few degrees Celsius and still have the same volume. The PRESSURE however will increase quite noticeably. If you just have the water in an open container and heat it several degrees Celsius, it will not have the same volume. Liquid water actually reaches its maximum density at about 4 °C where it has a density of 1000 kg/m3. Below that temperature, the density of liquid water decreases until it hits about 999.868 kg/m3 at 0 °C. Above 4 °C, the density also decreases. It doesn't reach the same density as 0 °C water until it has warmed to about 8.14 °C. Obviously, in that narrow range, it is possible to warm a sample of water several degrees Celsius and end with it being the same volume (but it wont have the same volume between the two temperatures).
468ml
The volume (at 20 degrees celsius and a pressure of 1 atmosphere) is 107.7mL. Both changes in temperature or pressure will change the answer.
136.73 mL
By decreasing the pressure with the volume kept constant.
By decreasing the pressure with the volume kept constant.
A fixed quantity of gas at a constant pressure exhibits a temperature of 27 degrees Celsius and occupies a volume of 10.0 L. Use Charles's law to calculate: the temperature of the gas in degrees Celsius in atmospheres if the volume is increased to 16.0 L
A sample of Ar gas occupies a volume of 1.2 L at 125°C and a pressure of 1.0 atm. Determine the temperature, in degrees Celsius, at which the volume of the gas would be 1.0 L at the same pressure.
1 mL
The melting temperature of a substance is dependent upon the pressure and specific volume. The melting temperature of liquid at standard pressure of 1atm (~100kPa) is 0 degrees Celsius.
25 ml. The volume would not change. Now pressure on the other hand...
P1V1/T1 = P2V2/T2Assuming only temperature and volume are changing and pressure will be kept constant:V1/T1 = V2/T2Only Kelvin can be usedV1/273 = V2/523Assume the volume at 0 ºC is 1 unit thenV2 = 1.92 units
P1V1/T1 = P2V2/T2Assuming only temperature and volume are changing and pressure will be kept constant:V1/T1 = V2/T2Only Kelvin can be usedV1/273 = V2/523Assume the volume at 0 ºC is 1 unit thenV2 = 1.92 units