Mass of unknown metal (metal x): 0.184g, Volume of H gas 82.1 mL, Temp H2 gas...
Mass of unknown metal (metal x): 0.184g, Volume of H gas 82.1 mL, Temp H2 gas 294.3K, partial pressure of H2 gas is 0.980 atm. Convert moles of H2 gas to moles of unknown metal X using the balanced equation X + 2HCl = XCl2 +H2 and calculate the molar mass of the metal. Please show work.
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Mass of unknown metal (metal x): 0.184g, Volume of H gas 82.1
mL, Temp H2 gas...
Experiment 12: Generating Hydrogen Gas Part B: Molar mass of unknown metal Unknown #: Mass of...
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...
Please do the following questions! thank you! Experiment 12: Generating Hydrogen Gas Part B: Molar mass...
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...
what's the difference between wet H2 and dry H2? V. DATA Insert data table prepared in...
what's the difference between wet H2 and dry H2?
V. DATA Insert data table prepared in pre-lab. Trial Mass Vfinal Vinitial Pressure Number Metal (g (ml) Vapor Pressure Pressure TH,。。C Temp (inHg) (mL) (torr) Value is found from standard table or meter VI. CALCULATIONS You must SHOW ALL WORK for calculations made in order to obtain a res guide your work but other calculations may be necessary in order to results clearly and always include units. substantiate results. Be sure...
2. A 0.865g sample of an unknown metal (X) reacted with hydrochloric acid according to the...
2. A 0.865g sample of an unknown metal (X) reacted with hydrochloric acid according to the balanced chemical equation shown below. XC12 (aq) + H2() X+ 2 HCl(q) The volume of the hydrogen gas collected over water was measured at 191 mL at 22C and an atmospheric pressure of 762 mmHg. Calculate the molar mass of the unknown metal, and use a periodic table to identify the metal. Molar mass: The metal is 127
Experiment 12. Generating Hydrogen Cas A. Percent yield of hydrogen gas Mass of magnesium -0.051 Volume...
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 ....
Experiment 12: Generating Hydrogen Gas Data: A. Percent yield of hydrogen gas Mass of magnesium 0.04298...
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...
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...
1) Given the following data, calculate the temperature of the gas in Kelvin, the pressure of the ...
1) Given the following data, calculate the temperature of the gas in Kelvin, the pressure of the gas in atm, the mass of the condensed liquid, the volume of the gas in L, the moles of gas in the flask and then calculate the molar mass of the unknown liquid Mass of empty flask and foil 78.639g 99.3°C 14.4 psi 79.118g Temperature of hot water atm Pressure in lab Mass of flask, foil and condensed unknown liquid AFTER heating and...
Magnesium metal reacts with hydrochloric acid to give hydrogen gas. Mg + 2 HCl → MgCl2...
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...
i need help with the moles of H2 gas please Trial 1 Trial 2 Mass of...
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 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...
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...
what's the difference between wet H2 and dry H2?
V. DATA Insert data table prepared in pre-lab. Trial Mass Vfinal Vinitial Pressure Number Metal (g (ml) Vapor Pressure Pressure TH,。。C Temp (inHg) (mL) (torr) Value is found from standard table or meter VI. CALCULATIONS You must SHOW ALL WORK for calculations made in order to obtain a res guide your work but other calculations may be necessary in order to results clearly and always include units. substantiate results. Be sure...
2. A 0.865g sample of an unknown metal (X) reacted with hydrochloric acid according to the balanced chemical equation shown below. XC12 (aq) + H2() X+ 2 HCl(q) The volume of the hydrogen gas collected over water was measured at 191 mL at 22C and an atmospheric pressure of 762 mmHg. Calculate the molar mass of the unknown metal, and use a periodic table to identify the metal. Molar mass: The metal is 127
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 ....
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...
1) Given the following data, calculate the temperature of the gas in Kelvin, the pressure of the gas in atm, the mass of the condensed liquid, the volume of the gas in L, the moles of gas in the flask and then calculate the molar mass of the unknown liquid Mass of empty flask and foil 78.639g 99.3°C 14.4 psi 79.118g Temperature of hot water atm Pressure in lab Mass of flask, foil and condensed unknown liquid AFTER heating and...
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...
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...
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