The vapor pressure of carbon tetrachloride is 11.94 Pa at 20°C
This is 0.0896 torr or 89.6 mTorr
To find the volume of dry hydrogen at STP, we need to correct for the presence of water vapor. First, calculate the pressure of dry hydrogen by subtracting the vapor pressure of water from the total pressure: 745.5 torr - 14.5 torr = 731 torr. Then, apply the ideal gas law to solve for the volume of dry hydrogen at STP: V = (200 ml * 731 torr * 273 K) / (290 K * 760 torr) ≈ 181 ml.
600 Torr (1 atm/760 Torr) = 0.789 atmospheres ================
The temperature of the water is 100 degrees celsius.
0.395 total moles moles F 760.torr 300.torr total moles moles F 2 2 = ×
To find the pressure of the hydrogen gas in torr, you can use the difference in height of the mercury columns and the density of mercury. First, calculate the pressure difference due to the 18.0 cm height difference in the mercury columns. Then, convert this pressure into torr using the conversion factor 1 atm = 760 torr.
The vapor pressure of pure water at 25 degrees Celsius is 23.8 torr.
To find the volume of dry hydrogen at STP, we need to correct for the presence of water vapor. First, calculate the pressure of dry hydrogen by subtracting the vapor pressure of water from the total pressure: 745.5 torr - 14.5 torr = 731 torr. Then, apply the ideal gas law to solve for the volume of dry hydrogen at STP: V = (200 ml * 731 torr * 273 K) / (290 K * 760 torr) ≈ 181 ml.
Turning ice into vapor in a vacuum chamber at 1 torr requires a lower pressure than standard atmospheric pressure to facilitate sublimation (ice directly turning into water vapor without melting). At 1 torr, the pressure might not be low enough to overcome the energy required for sublimation. Lower pressures, below 1 torr, are typically needed for efficient ice sublimation in a vacuum chamber.
Vapor pressure of a liquid at its normal boiling temperature is simply the atmospheric pressure, aka 1 atm, 760 torr, etc. This is by definition.
1075 torr - 720 torr = 355 torr
its the same 235 torr
630 torr
630 torr
We are considering the process: C2H5OH (l) -> C2H5OH (g) Kp = P(C2H5OH) At the normal boiling point of C2H5OH, the equilibrium constant, Kp, for this process is 1, and ΔG0 = -RTln(K) = 0 = ΔH0 - TΔS0. Substituting 42600 J for ΔH0 and 78.5 + 273.15 = 351.65 K for T gives ΔS0 = 121 J/K.
11,012 torr
600 Torr (1 atm/760 Torr) = 0.789 atmospheres ================
The vapor pressure of water at 72 degrees Celsius is approximately 28.1 mmHg.