Answer) According to Dalton's law
Ptotal = PH2O + PH2
PH2 = Ptotal - PH2O
= 759.2 torr - 23.7 torr
=735.5 torr
Question 3 0/1 pts If the pressure in the room is 759.2 Torr and the vapor...
The following data was obtained: atmospheric pressure: 752 torr water vapor pressure: 22 torr height of water column: 158 mm Calculate the partial pressure of the dry gas. Density of mercury if 13.6 g/cm3 and assume the desnity of the solution is 1.00 g/cm3/
during the analysis the barometric pressure was recorded to be 740 torr and the vapor pressure of water was 18.3 torr what will be pressure of dry CO2
A total of 0.829 L of hydrogen gas is collected over water at 33.0°C. The total pressure is 794 torr. If the vapor pressure of water at 33.0°C is 13.2 torr, what is the partial pressure of hydrogen? torr
confused about the wording on the first two calculations and what
to look for.
A. DATA 170 Trial 1 1. Mass of magnesium. 2. Calibration of gas measuring tube 3. Volume of gas in tube (mL) 4. Barometric pressure (torr) TITLULUUUUUUUUUU 0878 8704 2 anh 88.2m6 67.0me 710. Bruly 770.13 multy 14 Leden 135mm 2oc zdce 198 tot 22c 220 5. Height of water in the gas measuring tube above the water in the beaker (mm) 6. Room temperature (°C)...
question 3 pls
6. The vapor pressure of water at 20°C is 17.54 torr. Calculate the vapor pressure (in torr) of an aqueous solution containing 21.88 g of ethylene glycol (C H O2) in 71.22 g of water at 20°C.
1) At a temperature of torr °C, 0.444 mol of CO gas occupies 11.8 L at 839 2) Hydrogen gas is produced when aluminum reacts with hydrochloric acid: Al(s) + HCl(aq) AlCl3(aq) + H2(g) [Unbalanced] If 940.1 mL of wet hydrogen is collected over water at 23.7 °C and a barometric pressure of 748.69 torr, how many grams of Al have been consumed? (The vapor pressure of water at 23.7 °C is 21.98 mmHg) 3) Follow auf bau principle for...
A 1,096.9 mL sample of hydrogen gas was collected over water at 25°C and a pressure of 777.6 torr. If the pressure of water vapor is 24.0 torr at 25.0°C, what mass of hydrogen gas (g) was collected?
a sample of hydrogen gas is mixed with water vapor. the mixture has a total pressure of 755 torr and the water vapor has a partial pressure of 24 torr. what amount (in moles) of hydrogen gas is contained in 1.55 L of this mixture at 298 K?
1)The barometric pressure is reported to be 695.1 torr and the temperature of the water bath is 22.0 °C. What is the pressure (in torr) of dry hydrogen gas in the eudiometer? 2)Calculate the experimental value of the ideal gas constant, R, if 0.00148mol of hydrogen had a volume of 45.5mL at 22.8°C and 0.7771atm. Hint: remember to convert mL to L and °C to K Hint: Answer includes 3 significant figures.
The vapor pressure of pure water at 25.0 °C is 23.76 torr. The vapor pressure of a solution containing 5.40 g of a nonvolatile substance in 90.0 g of water is 23.32 torr. What is the molecular weight of the solute?