volume of eudiometer is not given. what do I do?
Percent Yield of Hydrogen Gas From Magnesium and HC PRESTUDY Nitrogen gas is collected over water...
TFW 5:38 PM X Yld H2FrmMgandHCI-1030-201 Name General Chemistry I Percent Yield of Hydrogen Gas From Magnesium and HCI PRESTUDY Nitrogen gas is collected over water in a eudiometer. The volume of the nitrogen gas is 125 mL the atmospheric pressure is 763 mm Hg, the water temperature is 24 °C, and the water level inside the eudiometer is the same as the level of water in the beaker 1. (2) Calculate the pressure of the dry nitrogen gas. For...
In an experiment, magnesium metal was dissolved in HCl and hydrogen gas was collected in an eudiometer. The hydrogen gas was mixed with water vapor. The mixture has a total pressure of 757 torrtorr , and the water vapor has a partial pressure of 23 torrtorr . What amount (in moles) of hydrogen gas is contained in 1.61 LL of this mixture at 298 KK? Express the amount in moles to three significant figures.
-REPORT FO SECTION DATA Mass of magnesium strip: 2402 Temperature of water from the thermometer: 71 3705 Atmospheric pressure (inches) 29.3Sx 2513 Volume of gas collected: CALCULATIONS: (Show work) 20 94A0つ Moles of magnesium: OS10X 24.30 2.094316 3 Moles of hydrogen produced 12 29215K Temperature of gas in Kelvins: Volume of hydrpgen gas in liters: Atmospheric pressure (mm. Hg): Vapor pressure of water in eudiometer: Pressure of hydrogen gas in eudiometer (mm.Hg.): Pressure of hydrogen gas (atmosphere): Calculated value of...
3. Nitrogen gas was collected in a eudiometer during a chemistry experiment by displacement of water. When the levels of water inside and outside the eudiometer were adjusted to be the same, the volume of the collected gas was found to be 85.2 mL. The water temperature was 24°C and the barometric (atmospheric) pressure was found to be 764.0 mm Hg. What would be the volume of dry nitrogen gas at STP?
A nitrogen sample occupies 201 mL at STP. If the same sample were collected over water at 25°C and 700. torr, what would be the volume of the gas sample? (Assume that vapor pressure of water at 25°C is 23.8 torr.)
A volume of 30.0 mL of nitrogen gas was collected over water at 24.0°C and 0.98 atm. The vapor pressure of water at this temperature is 0.03 atm. a. What is the partial pressure of the nitrogen gas sample, (use Dalton's law)? b. What would the new volume of this gas be at STP. (Use the combined gas law)?
3. A volume of 30.0 mL of nitrogen gas was collected over water at 24.0°C and 0.98 atm. The vapor pressure of water at this temperature is 0.03 atm. a. What is the partial pressure of the nitrogen gas sample, (use Dalton's law)? b. What would the new volume of this gas be at STP. (Use the combined gas law)?
Mass of Magnesium Volume of gas produced Height of water column Trial 2 0.03029 Trial 1 0.03309 34.4mL 18.26cm 21.7 mmity 23.5°C 751 torr Pressure of water column Temperature of water Atmospheric pressure 23.76 mm Hg 25.0°c 751 torr Water vapor pressure CALCULATIONS: Perform calculations for both trials. 1. Calculate the total pressure of the gases inside the eudiometer at the end of the experiment. Trial 1 Trial 2 2. Calculate the partial pressure of the hydrogen gas in the...
a) A sample of oxygen gas is collected by displacement of water at 25°C and 1.13 atm total pressure. If the vapor pressure of water is 23.756 mm Hg at 25°C, what is the partial pressure of the oxygen gas in the sample? WebAssign will check your answer for the correct number of significant figures. mm Hg b) Calcium oxide can be used to "scrub" carbon dioxide from air. CaO(s) + CO2(g) → CaCO3(s) What mass of CO2 could be...
QUESTION 3 A student collected a sample of hydrogen gas in a eudiometer over a water bath to experimentally determine the value of the gas constant, R. Calculate the experimental value of Rif the pressure of the gas was 0.991 atm, the volume was 36.3 mL the temperature was 292 K and the sample contained 1.54 x 103 moles of gas. QUESTION 4 A student collected a sample of hydrogen gas in a eudiometer over a water bath. The atmospheric...