Pressue and Temperature are same for both traails
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1 mole of Mg liberates 1 mole of Hydrogen gas.
24 g of Mg liberates 2 g of hydrogen gas in mass terms.
0.031 g of Mg liberates how much hydrogen gas= ?
Mass of hydrogen released in Trail 1 = ( 0.031 g * 2 g ) / 24 g
= 0.00258 g
Moles of Hydrogen gas = 0.00258 g/ 2 g/mol
= 0.00129 mol of Hydrogen
value of Gas constant, R is derived by Ideal gas equation -----
pV = nRT
R = pV/nT
T = 293.25 K ( 20.1 ^oC +273.15)
pressure of dry hydrogen gas , P = 767.4 mm- 17.5 mm
= 749.9 mm
=( 749.9/760 ) atm
= 0.987atm
volume of gas = 30.70 ml
= 0.0307 L
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R = pV/nT
= 0.987 atm * 0.0307 L ) / 0.00129 mol * 293.25 K
= 0.080 Lit.atm/K.mol --------------------------------------------------------------------trail 1
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1 mole of Mg liberates 1 mole of Hydrogen gas.
24 g of Mg liberates 2 g of hydrogen gas in mass terms.
0.042 g of Mg liberates how much hydrogen gas= ?
Mass of hydrogen released in Trail 2 = ( 0.042 g * 2 g ) / 24 g
= 0.0035 g
Moles of Hydrogen gas = 0.0035 g/ 2 g/mol
= 0.00175 mol of Hydrogen
value of Gas constant, R is derived by Ideal gas equation -----
pV = nRT
R = pV/nT
T = 293.25 K ( 20.1 ^oC +273.15)
pressure of dry hydrogen gas , P = 767.4 mm- 17.5 mm
= 749.9 mm
=( 749.9/760 ) atm
= 0.987atm
volume of gas = 43.05 ml ml
= 0.04305 L
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R = pV/nT
= 0.987 atm * 0.04305 L ) / 0.00175 mol * 293.25 K
= 0.0828 Lit.atm/K.mol -------------------------------------------------------------------------trail 2
9->moles Data Table - Mg with HCI nga2 + H₂ Ptoral - Plzo =PHz Trial 1...
Data Collecting hydrogen gas from the reaction of Mg with HCI Trial 1 Trial 2 Trial 3 Atmospheric pressure (in Hg) O pen Mass Mg ribbon 0.069 1.osa. 1.069 Volume Ha collected (ml) sim 40 mL de ML Temperature of water (°C) 23 с әət 1 22oC Vapor pressure of water (Table 10.1) 19.8WHO 19.8 mmHg 1.8 in Ho Atmospheric pressure (mm Hg) Partial pressure of H2 Temperature of water (K) Volume of H: collected (L) Moles Hz Theoretical moles...
moles of Mg and balanced chenical reactions with phases
Name: Haytry Stonavina Data Section #: Date: Collecting hydrogen gas from the reaction of Mg with HCI TO HG Atmospheric pressure in Hg) Mass Mg ribbon Volume Ha collected (ml) Temperature of water (°C) 11 Partial pressure of H: Temperature of water (K) Trial 1 Trial 2 Trial 3 1 7600 nano 700 ruilo osolog .059 1.089 sime 46 ML I de ML 22°C 22°C 12°c 19.8 mmHg 19.8 amHg 19.8...
moles of Mg reacted for Trial 1 and Trial 2. show
calculations
Trial Trial 1 Measured Data 0.04 43,7 mL F4h mmHg Mass of Mg (g) (2pts) Volume of H2 gas (mL) (4pts) 44.3 ml Barometric Pressure (mm Hg) (2pts) (i.e., Atmospheric Pressure) Temperature (°C) (3pts) Calculations: Moles of Mg reacted (4pts) Show Calculations: (2)
Experiment 12: Generating Hydrogen Gas Data: A. Percent yield of hydrogen gas Mass of magnesium 0.04298 Volume of H2 gas (actual) 42.ml 0.0426 24.0°C 297 Temperature of H, gas Atmospheric pressure (see barometer) 765.8 mmHg a2.4 mmHg Vapor pressure of water Partial pressure of Hą gas 743.4 mmHg 0.976 1 atm Calculate the moles of hydrogen gas that should have been produced, starting with the mass of Mg and using the balanced equation. mg = 24.31 Mg(s) + 2 HCI...
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...
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...
Experiment 12. Generating Hydrogen Cas A. Percent yield of hydrogen gas Mass of magnesium -0.051 Volume of gas (actual) Temperature of H gas Atmospheric pressure (see barometer) 20 °C 24 mmHg 26PmHg mmHg Vapor pressure of water there mmtig Partial pressure of He gas Calculate the moles of hydrogen gas that should have been produced, starting with the mass of Mg and using the balanced equation. Mg (8) + 2 HCI (aq) → MgCl(aq) + H2 (8) 0.08ling Imoling ....
Section - Date Name Lab Partner DATA Trial Mass of Mg (g) - 0.0301 3 Temperature (°C) Volume of H, gas (mL) 30.1 Barometric Pressure (mmHg)_latm 349 38.6 lamm CALCULATIONS A. Experimental Determination of the gas constant, R 1. Write the balanced chemical equation for the reaction between magnesium and hydrochloric acid 2. How many moles of Mg were consumed? 3. Based upon the chemical equation how many moles of H, gas were produced? 4. What volume of H, gas...
DATA TABLE Trial 1 Trial 2 Mass of Erlenmeyer flask, rubber band and foil cover (g) 90.560 90.10 Temperature of water bath (°C) 100t 99.1 Mass of Erlenmeyer flask, rubber band, foil cover and condensed 0819 gas sample (9) Mass of the condensed gas sample (9) 251.59 Barometric (atmospheric) pressure (mmHg) 128.96 28.93 Volume of the Erlenmeyer flask (mL) 170 170 Molar mass of the unknown sample (g/mole) Average molar mass (g/mol): DATA ANALYSIS (Show your calculations) 1. Determine the...
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...