what's the difference between wet H2 and dry H2?
In the given experiment, metal reacts with acid and the H2 gas produced is collected by the displacement of water.Hence the gas collected is a mixture of H2 gas and water vapor which is termed as "wet gas" and the pressure obtained will be pressure of H2 gas + partial vapor pressure of water at the same temperature.(Aqueous tension)
Dry H2 gas is the gas without water vapor.
Pressure of dry H2 gas = Observed pressure - Aqueous tension.
In the given experiment, metal reacts with acid and the H2 gas produced is collected by the displacement of water.Hence the gas collected is a mixture of H2 gas and water vapor which is termed as "wet gas" and the pressure obtained will be pressure of H2 gas + partial vapor pressure of water at the same temperature.(Aqueous tension)
Dry H2 gas is the gas without water vapor.
Pressure of dry H2 gas = Observed pressure - Aqueous tension.
what's the difference between wet H2 and dry H2? V. DATA Insert data table prepared in...
A student performed an experiment in which hydrogen gas was collected over water from the reaction of magnesium and hydrochloric acid using the apparatus shown and accoridng to the reaction equation and the data collected shown below: Mass of Mg 0.100 g Volume of HCl 10 mL Volume of H2 collected 57.5 mL Temperature of H2 collected 22.0 oC Barometric pressure 29.94 inHg Mg(s) + 2 HCl(aq) → H2(g) + MgCl2(aq) a. Barometric pressure in atmospheres? b. Water vapor pressure...
The Atomic Weight of a Metal Data Trial 2 Trial 1 .036a 37.3mL 22.8°C 33.5ml 22. 2°C 1. Mass of Magnesium (g) 2. Volume of Hydrogen Gas Collected (mL) 3. Temperature (°C) 4. Temperature (K) (show calculation) 5. Barometric Pressure (mm Hg) Height Difference between Water Levels (mm H,O) tin loin Mercury Equivalent of Height Difference Water Difference (show calculation) 13.6 Vapor Pressure of Water (will be given-mm Hg) Pressure of Dry Hydrogen Gas = Barometric Pressure - Mercury Equivalent...
DATA Trial 1 Trial 2 Mass of Mg ribbon (g) TO SU 0.07839 (Proom) Barometric pressure (mmHg) 756 matte 756rrotta | 22.4°C Temperature of water inside beaker (C) 23.0°C 22.8°C Temperature of the room (°C) (T2) Pwater (mm Hg) Vapor pressure of water found in table at the end of the experiment, based on the temperature of water inside the beaker. 5 mm Hg Volume from graduated cylinder (mL) (V2) 60.2mL 82.4mL CALCULATIONS . Write the balanced chemical equation for...
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 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 overwater the data is complied in the table total volume of H2(g) collected = 96.41 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
Experimental Determination of the Gas Constant Experimental Data . (a) Mass of Magnesium metal used (b) Volume of H, gas collected mi (C) Temperature of H2 gas collected (d) Atmospheric Pressure (e) Temperature of Water in bath (bucket) Vapor Pressure of Water at above temperature Trial 0.03419 36.0 ml 22 • 766-5 mm/Hg 2214 oc 19.3 mmHg Trial 2 0.02129 20.5 mL 23-0's 766 5mnHg 224 °C 22 mmHg Data Analysis Using your experimental data, determine the value of R,...
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
drogen produced from a hydrolysis reaction was collected over water. The data is compiled in the table. Total volume of H2(g) collected Temperature Barometric pressure Vapor pressure of water at 27.0°C 95.18 ml 27.0°C 737 mmHg 27.0 mmHg Calculate the moles of hydrogen gas produced by the reaction. moles: mol H
i need help with the moles of H2 gas please Trial 1 Trial 2 Mass of Mg ribbon (e) 10.0541 g 0.07839 Barometric pressure (mmHg) (Proom) 1 75 66 matts 756 mutta Temperature of the room (°C) 224 °C 22.4 °C Temperature of water inside beaker (°C) 23.0°C 22.8°C (T2) Pwater (mm Hg) Vapor pressure of water found in table 21.068 van Hg 20.615 mm Hg at the end of the experiment, based on the temperature of water inside the...