PV/T=Constant
Providing the volume remains constant.
P/T=C
35/313=20/T
Therefore T=178.9Kelvin
Determine the specific heat of a material if a 32 g sample of the material absorbs 58 J as it is heated from 298 K to 313 K?
The boiling point of carbon dioxide is -57 °C (or 216.6 K, or -70 °F), but this will only take place at pressures in excess of 5.1 atmospheres. It turns out that CO2 doesn't like to hang around in liquid form unless it is under a good deal of pressure. It will sublime (change directly from a gas into a solid) at anything above −78 °C, and deposit directly as a solid from the gas at anything below −78 °C. In environments without elevated pressure, it changes state from solid to gas and gas to solid (depending on temperature) directly without going through a liquid phase.Added:At 1.0 bar, normal pressure, it sublimes (solid-gas phase change) at -78 °C, 194.7 K without passing through its liquid phase.At 5.185 bar the boiling point (from liquid) is -57 °C, 216.6 K.
The address of the Sun Prairie Historical Society Inc is: Po Box 313, Sun Prairie, WI 53590
Gamma rays from uranium-238: * 0,013 000 MeV energy and 0,088 313 probability * 0,066 376 MeV energy and 0,000 970 probability
39000 sq. ft = 0.901442 acres.
313 Kelvin.
The pressure inside a CO2 extinguisher can vary depending on the temperature. Assuming it starts at room temperature, the pressure would increase as the cylinder is exposed to direct sunlight at 50°C. However, without further information, it is difficult to determine the exact pressure increase. It is important to note that CO2 extinguishers have pressure relief valves to prevent over-pressurization.
At normal pressure steam changes to liquid water at 212 degree F.
1 and 313 (313 is a prime number).
313 is a prime so radical 313 cannot be simplified.
97969
Moles Cl2 = 25g x 1mol/71g 0.35 molesPV =nRT and T = PV/nR T = (1.5)(6)/(0.35)(.0821) T = 313 deg K = 40.2 deg C to 3 sig figs
Using the ideal gas law (PV=nRT), you can calculate what would happen by just raising the temperature. Note that the T is in degrees Kelvin, so you would have to convert from C. V is the volume, n is the number of molecules and R is the gas constant, so those values would not change in your scenaro. From that, you can use: P2 = P1 * (T2 / T1): P2 = 2 * (313/288) P2 = 2.17 bar Note that this won't be exactly what occurs, but it gives you a close approximation. ("Impurities" in air will cause variations in the pressure rise. Moisture probably has the biggest effect, and it will typically increase the pressure rise. This is one of the reasons why nitrogen is being touted as "better than air" for your car tires.) Also, please note that the air pressure recommendations are for *cold* tires (i.e., at outside air temperature), so don't adjust for what you think the tire temperature may go up to.
It is: 334 -313 = 21
x x 313 = (x)(313) = 313x
127
The answer should be 2x-313