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Experiment 12: Generating Hydrogen Gas Part B: Molar mass...
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...
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...
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 8 Ideal Gas Law: Estimation of Molar Mass of Mognesium 57 QUESTIONS POST LAB A...
Experiment 8 Ideal Gas Law: Estimation of Molar Mass of Mognesium 57 QUESTIONS POST LAB A 0.0524-g sample of magnesium is reacted with 25 ml of 3.0 M sulfuric acid as described in the tal section. The resulting hydrogen gas is collected over water and is found to have a volume of 536 m m temperature is 25 °C and the atmospheric pressure is 762.12 mm Hg. The column of water height inside the graduated cylinder is found to be...
In the first cell, 42.51 mL of hydrogen gas were formed at the cathode.The temperature was...
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...
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.
Chame nsead tu age 06-17 Experiment 8: Molar Mass of a Volatile Liquid Purpose To determine...
Chame nsead tu age 06-17 Experiment 8: Molar Mass of a Volatile Liquid Purpose To determine the molar mass of a pure substance we need to find out (a) the number of moles in a given sample, and (b) the mass of the same sample. Molar mass is then: mass divided by moles Introduction Using the ideal gas equation, PV= nRT, we can determine the number of moles (n) of gas or vapor under measured conditions of pressure (P), volume...
Please answer whole page dent performed the experiment and obtained the following data. Convert the measurements...
Please answer whole page
dent performed the experiment and obtained the following data. Convert the measurements to the proper units. 22.0°c Trial 1 Mass of metal 0.048 g Volume of hydrogen gas 58.70 mL L= V, Temperature of gas K=T Atmospheric pressure 705.6 mmHg = atm (Vapor pressure of water 19.8 mmHg atm 1. Calculate the partial pressure for H, gas in units of atmospheres. Use Dalton's Law of Partial Pressures Atmospheric pressure - Vapor pressure of HO Partial pressure...
Please answer number1 0.3901.96 -0.00L592 miles MASS OF METAL PLACED IN CAPSULE VAPOR PRESSURE OF WATER...
Please answer number1
0.3901.96 -0.00L592 miles MASS OF METAL PLACED IN CAPSULE VAPOR PRESSURE OF WATER TRIAL 1 TRIAL 2 0, 100 g 21.1 mm Hg ATMOSPHERIC PRESSURE 755. 65 mm Ho MOLES H2 EVOLVED 0.00 6822 moles EQUIVALENT MASS OF METAL 549, 05 g % ERROR st (need extact number) 3 metal ego. mass = 6.94 glad LiL Hinmole H gx 22 Pa- 20.00 6322 med Ha V-nb bau.na = 549:05 g as out UESTIONS (Read textbook TRO chapter...
57 ldeal Gas Law: Estimation of Molar Mass of Magnesium Experiment 8 QUESTIONS A POST LAB...
57 ldeal Gas Law: Estimation of Molar Mass of Magnesium Experiment 8 QUESTIONS A POST LAB A 0.0524-g sample of magnesium is reacted with 25 mL of 3.0 M sulfuric acid as described in the experimen- tal section. The resulting hydrogen gas is colllected over water and is found to have a volume of 53.6 mL. The temperature is 25 °C and the atmospheric pressure is 762.12 mm Hg. The column of water height inside the graduated cylinder is found...
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...
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...
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 8 Ideal Gas Law: Estimation of Molar Mass of Mognesium 57 QUESTIONS POST LAB A 0.0524-g sample of magnesium is reacted with 25 ml of 3.0 M sulfuric acid as described in the tal section. The resulting hydrogen gas is collected over water and is found to have a volume of 536 m m temperature is 25 °C and the atmospheric pressure is 762.12 mm Hg. The column of water height inside the graduated cylinder is found to be...
Chame nsead tu age 06-17 Experiment 8: Molar Mass of a Volatile Liquid Purpose To determine the molar mass of a pure substance we need to find out (a) the number of moles in a given sample, and (b) the mass of the same sample. Molar mass is then: mass divided by moles Introduction Using the ideal gas equation, PV= nRT, we can determine the number of moles (n) of gas or vapor under measured conditions of pressure (P), volume...
Please answer whole page
dent performed the experiment and obtained the following data. Convert the measurements to the proper units. 22.0°c Trial 1 Mass of metal 0.048 g Volume of hydrogen gas 58.70 mL L= V, Temperature of gas K=T Atmospheric pressure 705.6 mmHg = atm (Vapor pressure of water 19.8 mmHg atm 1. Calculate the partial pressure for H, gas in units of atmospheres. Use Dalton's Law of Partial Pressures Atmospheric pressure - Vapor pressure of HO Partial pressure...
Please answer number1
0.3901.96 -0.00L592 miles MASS OF METAL PLACED IN CAPSULE VAPOR PRESSURE OF WATER TRIAL 1 TRIAL 2 0, 100 g 21.1 mm Hg ATMOSPHERIC PRESSURE 755. 65 mm Ho MOLES H2 EVOLVED 0.00 6822 moles EQUIVALENT MASS OF METAL 549, 05 g % ERROR st (need extact number) 3 metal ego. mass = 6.94 glad LiL Hinmole H gx 22 Pa- 20.00 6322 med Ha V-nb bau.na = 549:05 g as out UESTIONS (Read textbook TRO chapter...
57 ldeal Gas Law: Estimation of Molar Mass of Magnesium Experiment 8 QUESTIONS A POST LAB A 0.0524-g sample of magnesium is reacted with 25 mL of 3.0 M sulfuric acid as described in the experimen- tal section. The resulting hydrogen gas is colllected over water and is found to have a volume of 53.6 mL. The temperature is 25 °C and the atmospheric pressure is 762.12 mm Hg. The column of water height inside the graduated cylinder is found...
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