In the first cell, 42.51 mL of hydrogen gas were formed at the cathode.The temperature was 21.5C and the vapor pressure of water at this temperature is 19.240 torr. The Barometric pressure was 758.8 mm Hg and the height of water in the buret above the level of water in the beaker was 8.2 cm.
Calculate:
a. Partial Pressure of Hydrogen (H2) in buret (PH2 =
Barometric – VP – Pheight)
(The pressure due to the height of water still in the buret is a
conversion frommmH2O to mmHg. Since the density of water is 1.00
g/mL and the density of mercury is 13.6 g/mL, Pheight in mmHg =
(Height in mm)*(1.00/13.6))
b. Moles of Hydrogen (H2) gas formed (PV = nRT) (R =
0.08206 (L atm)/(K mol) = 62364 (mL torr)/(K mol))
c. Number of Faradays (= moles of electrons) that passed through
the cell using the conversion (2 mol e- per 1 mol H2)
In the first cell, 42.51 mL of hydrogen gas were formed at the cathode.The temperature was...
2 Calculate the pressure of the Hydrogen gas collected. Water temperature was 23.0 ° C and the atmospheric pressure was 741.0 mmHg. (Hint the density of Mercury is 13.6 g/mL) H2 gas collected over water 220. mm H20 RT
Experiment 12: Generating Hydrogen Gas Part B: Molar mass of unknown metal Unknown #: Mass of unknown metal (X) .29 Volume of H2 gas L mL Temperature of H; gas 20 mm к C Atmospheric pressure (see barometer) Vapor pressure of water mmHg Partial pressure of H; gas mmHg atm Using PV-nRT and your data, calculate the moles of hydrogen gas produced in the experiment: l e epl8 moles H Convert moles of hydrogen gas to moles of the metal...
Hydrogen produced from a hydrolysis reaction was collected over water. The data is compiled in the table. Total volume of H2(g) collected 95.06 mL Temperature 24.0 °C Barometric pressure 743 mmHg Vapor pressure of water at 24.0 °C 22.5 mmHg Calculate the moles of hydrogen gas produced by the reaction. moles: moles: mol H2 mol H,
Hydrogen produced from a hydrolysis reaction was collected over water. The data is compiled in the table. Total volume of H2(g) collected 96.96 mL Temperature 25.0°C Barometric pressure 742 mmHg Vapor pressure of water at 25.0°C 24.0 mmHg Calculate the moles of hydrogen gas produced by the reaction. moles: mol H2
Magnesium metal reacts with hydrochloric acid to give hydrogen gas. Mg + 2 HCl → MgCl2 + H2 Use the following reaction information to answer the subsequent questions. Show all of your work. 92 mm Length of Magnesium ribbon: Barometric Pressure: 762.9 mmHg Water Temperature: 29 °C Initial Gas Volume: 0.00 mL Final Gas Volume: 67.35 mL 0.7559 Mass = Length (in mm) x (1000 mm) 1. Magnesium is usually found in the laboratory as a ribbon strip. Find the...
Please do the following questions! thank you! Experiment 12: Generating Hydrogen Gas Part B: Molar mass of unknown metal Unknown #: Mass of unknown metal (X): Volume of H2 gas L K Temperature of H2 gas 0.12588 54.4 mL 23.0 C 765.8 mmHg 21.1 mmHg 744.7 mmHg Atmospheric pressure (see barometer) Vapor pressure of water atm Partial pressure of H, gas Using PV=nRT and your data, calculate the moles of hydrogen gas produced in the experiment: PV = 0.97987x54.4xio RT...
Taking into account the vapor pressure of water, how many moles of hydrogen gas, n, are present in 343 mL at 752 torr and 29 ∘C?The value of the gas constant R is 0.08206 L⋅atm/(mol⋅K). You may also find the conversion factors 1 atm=760 torr and TK=TC+273 useful. Express the number of moles to three significant figures.
Hydrogen produced from a hydrolysis reaction was collected over water. The data is compiled in the table. Total volume of H2(g) collected 94.91 mL 28.0 °C Temperature Barometric pressure 744 mmHg Vapor pressure of water at 28.0 °C 28.5 mmHg Calculate the moles of hydrogen gas produced by the reaction moles: 327.897 mol H2
Hydrogen produced from a hydrolysis reaction was collected over water. The data is compiled in the table. Total volume of H2(g) collected 96.02 mL. Temperature 23.0°C Barometric pressure 735 mmHg Vapor pressure of water at 23.0 °C 21.0 mmHg Calculate the moles of hydrogen gas produced by the reaction. moles: mol
Hydrogen produced from a hydrolysis reaction was collected over water. The data is compiled in the table. Total volume of H2(g) collected 93.33 mL Temperature 26.0 °C Barometric pressure 735 mmHg Vapor pressure of water at 26.0 °C 25.5 mmHg Calculate the moles of hydrogen gas produced by the reaction. moles: mol H 2