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Mass of Magnesium moles of magnesium = moles of H₂ mass of magnesium = moles of magnesium x (24.31 g/mol) Percent Error Percent Error= I(mass of magnesium from H₂)-(mass of magnesium from balance) | (mass of magnesium from balance) Record the percent error for each run on the RESULTS sheet. DATA Make sure to use correct significant figures and units of measure. 747 MM barometric pressure: Run 1 mass of magnesium strip: temperature of water: 16.48° volume of H₂ gas: 62ML height of water column: 230 ML 58 Run 2 g Run 2 mass of magnesium strip: 0.53g temperature of water: 1648° volume of H₂ gas: M( height of water column: 270 ML Run 3 mass of magnesium strip: 061 temperature of water: 16.480 59ML volume of H₂ gas: height of water column: 250ML 23 X 10 = 230 27 Xlos 270 * 100% ·08211004.481-00-11 vapor pressure of water: 16.48 vapor pressure due to water column: 19.853 mmHg 0.935L MMH pressure of H₂: O. 1000 volume of H₂: 0,065 +273 temperature of H₂:289.48 moles of H₂:0 mass of Mg: percent error: (0.935) (0.065) (0.0821) (289.48) = 8,0025 y betwe

Mass of Magnesium moles of magnesium = moles of H₂ mass of magnesium = moles of magnesium x (24.31 g/mol) Percent Error Percent Error= I(mass of magnesium from H₂)-(mass of magnesium from balance) | (mass of magnesium from balance) Record the percent error for each run on the RESULTS sheet. DATA Make sure to use correct significant figures and units of measure. 747 MM barometric pressure: Run 1 mass of magnesium strip: temperature of water: 16.48° volume of H₂ gas: 62ML height of water column: 230 ML 58 Run 2 g Run 2 mass of magnesium strip: 0.53g temperature of water: 1648° volume of H₂ gas: M( height of water column: 270 ML Run 3 mass of magnesium strip: 061 temperature of water: 16.480 59ML volume of H₂ gas: height of water column: 250ML 23 X 10 = 230 27 Xlos 270 * 100% ·08211004.481-00-11 vapor pressure of water: 16.48 vapor pressure due to water column: 19.853 mmHg 0.935L MMH pressure of H₂: O. 1000 volume of H₂: 0,065 +273 temperature of H₂:289.48 moles of H₂:0 mass of Mg: percent error: (0.935) (0.065) (0.0821) (289.48) = 8,0025 y betwe

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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I need help with run 2 the last three parts
ALCULATIONS Water Vapor Pressure Use the temperature of water from Run 1 to find the corresponding vapor pressure of water in Table 1. Record this vapor pressure (in mmHg) on the RESULTS sheet. Find the vapor pressure in the same way for Run 2 and 3. Record these values on the RESULTS sheet. 230 13.6 = 16.912 Pressure due to Water Column 230ML Pressure (in mmHg) due to water column = (height of water column in mm)/13.6 Find the pressure due to water column for each run and record these values on the RESULTS sheet. Pressure of H₂ 16.48 16.912 247 Pressure of H₂ gas = (barometric pressure) - (vapor pressure of water) - (pressure due to water column) Find the pressure of H₂ (in mmHg) for each run, convert to atm, then record each on the RESULTS sheet. Volume of H₂ The volume of H₂ was determined in milliliters for each run. Convert these volumes to liters and record these values on the RESULTS sheet. Temperature of H₂ The temperature of the H₂ gas is the same as the temperature of water for each run. Convert each temperature to Kelvins, then record these values on the RESULTS sheet. Moles of H₂ 16.912x! 760 For each calculation, use the values of pressure, volume and temperature you've just recorded on the RESULTS sheet. They now have the proper units of measure to be used in the ideal gas law. (pressure of H₂)(volume of H₂) (0.0821 L-atm/K-mol)(temperature of H₂) Record the moles of H₂ for each run on the RESULTS sheet. moles of H₂ 5 -=0.022
Transcribed Image Text:ALCULATIONS Water Vapor Pressure Use the temperature of water from Run 1 to find the corresponding vapor pressure of water in Table 1. Record this vapor pressure (in mmHg) on the RESULTS sheet. Find the vapor pressure in the same way for Run 2 and 3. Record these values on the RESULTS sheet. 230 13.6 = 16.912 Pressure due to Water Column 230ML Pressure (in mmHg) due to water column = (height of water column in mm)/13.6 Find the pressure due to water column for each run and record these values on the RESULTS sheet. Pressure of H₂ 16.48 16.912 247 Pressure of H₂ gas = (barometric pressure) - (vapor pressure of water) - (pressure due to water column) Find the pressure of H₂ (in mmHg) for each run, convert to atm, then record each on the RESULTS sheet. Volume of H₂ The volume of H₂ was determined in milliliters for each run. Convert these volumes to liters and record these values on the RESULTS sheet. Temperature of H₂ The temperature of the H₂ gas is the same as the temperature of water for each run. Convert each temperature to Kelvins, then record these values on the RESULTS sheet. Moles of H₂ 16.912x! 760 For each calculation, use the values of pressure, volume and temperature you've just recorded on the RESULTS sheet. They now have the proper units of measure to be used in the ideal gas law. (pressure of H₂)(volume of H₂) (0.0821 L-atm/K-mol)(temperature of H₂) Record the moles of H₂ for each run on the RESULTS sheet. moles of H₂ 5 -=0.022
Mass of Magnesium moles of magnesium = moles of H₂ mass of magnesium = moles of magnesium x (24.31 g/mol) Percent Error Percent Error= I(mass of magnesium from H₂)-(mass of magnesium from balance) | (mass of magnesium from balance) Record the percent error for each run on the RESULTS sheet. DATA Make sure to use correct significant figures and units of measure. 747 MM barometric pressure: Run 1 mass of magnesium strip: temperature of water: 16.48° volume of H₂ gas: 62ML height of water column: 230 ML 58 Run 2 g Run 2 mass of magnesium strip: 0.53g temperature of water: 16.48° volume of H₂ gas: M( height of water column: 270 ML Run 3 mass of magnesium strip: 061 temperature of water: 16.480 59ML volume of H₂ gas: height of water column: 250ML 23 X|G = 230 27 xlos 270 * 100% ·08211004.481-00-17 vapor pressure of water: 6.48 vapor pressure due to water column: 19.853 mmHg 0.935L MMH pressure of H₂: O. 1000 volume of H₂: 0,065 +273 temperature of H₂:289.48 moles of H₂:0 mass of Mg: percent error: (0.935) (0.065) (0.0821) (289.48) = 8,0025 y betwe
Transcribed Image Text:Mass of Magnesium moles of magnesium = moles of H₂ mass of magnesium = moles of magnesium x (24.31 g/mol) Percent Error Percent Error= I(mass of magnesium from H₂)-(mass of magnesium from balance) | (mass of magnesium from balance) Record the percent error for each run on the RESULTS sheet. DATA Make sure to use correct significant figures and units of measure. 747 MM barometric pressure: Run 1 mass of magnesium strip: temperature of water: 16.48° volume of H₂ gas: 62ML height of water column: 230 ML 58 Run 2 g Run 2 mass of magnesium strip: 0.53g temperature of water: 16.48° volume of H₂ gas: M( height of water column: 270 ML Run 3 mass of magnesium strip: 061 temperature of water: 16.480 59ML volume of H₂ gas: height of water column: 250ML 23 X|G = 230 27 xlos 270 * 100% ·08211004.481-00-17 vapor pressure of water: 6.48 vapor pressure due to water column: 19.853 mmHg 0.935L MMH pressure of H₂: O. 1000 volume of H₂: 0,065 +273 temperature of H₂:289.48 moles of H₂:0 mass of Mg: percent error: (0.935) (0.065) (0.0821) (289.48) = 8,0025 y betwe
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