Weight of empty 125 ml Erlenmeyer flask = 88.9 g Weight of Erlenmeyer flask with water...

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Weight of empty 125 ml Erlenmeyer flask = 88.9 g Weight of Erlenmeyer flask with water filled to the neck = 237 g Data Table (Mg) Mass of Mg (g) Volume of flask (ml) Maximum pressure (kPa) Initial pressure (kPa) Pressure change, Delta P (kPa) Temperature (K) Data Table (Unknown) Mass of unknown metal (g) Volume of flask (ml) Maximum pressure (kPa) Initial pressure (kPa) Pressure change, Delta P (kPa) Temperature (K) Trial 1 0.014 125.0 118.0 101.0 17.1 Table 1 296 Trial 1 0.03 125.0 114.0 101.0 13.1 Table 2 296 Trial 2 0.012 125.0 115.0 101.0 14.1 Trial 2 296 0.03 125.0 107.0 101.0 6.2 297 Trial 3 0.014 125.0 111.0 101.0 10.3 296 Trial 3 0.03 125.0 106.0 101.0 4.7 296 Data Analysis: 1. Using the measured weight of the empty 125 mL weight when filled with water, and the known density of water at the temperature of the measurement, calculate the "effective" volume of the 125 mL Erlenmeyer flask, i.e., the volume available for occupancy by the H₂ gas. (You must also take into account the volume of the added HCl solution, which decreases the volume available to the H2 gas.) 2. Calculate the molar amounts of each piece of magnesium and unknown metal that you used. ENEW 3. Based on the measured temperatures and pressure changes for each reaction, use the ideal gas the molar amount of hydrogen gas that was produced in each reaction. 4. Calculate the volume occupied by one mole of hydrogen gas (molar volume) at STP. 5. Compare your calculated molar volume, at STP, with the accepted molar volume of an ideal gas at STP, viz., 22.41 L/mol. If the values do not compare well, suggest possible sources of experimental error. 6. Use your calculated value for the STP molar volume to determine the atomic weight of your unknown metal. What is the likely identity of the metal? Weight of empty 125 ml Erlenmeyer flask = 88.9 g Weight of Erlenmeyer flask with water filled to the neck = 237 g Data Table (Mg) Mass of Mg (g) Volume of flask (ml) Maximum pressure (kPa) Initial pressure (kPa) Pressure change, Delta P (kPa) Temperature (K) Data Table (Unknown) Mass of unknown metal (g) Volume of flask (ml) Maximum pressure (kPa) Initial pressure (kPa) Pressure change, Delta P (kPa) Temperature (K) Trial 1 0.014 125.0 118.0 101.0 17.1 Table 1 296 Trial 1 0.03 125.0 114.0 101.0 13.1 Table 2 296 Trial 2 0.012 125.0 115.0 101.0 14.1 Trial 2 296 0.03 125.0 107.0 101.0 6.2 297 Trial 3 0.014 125.0 111.0 101.0 10.3 296 Trial 3 0.03 125.0 106.0 101.0 4.7 296 Data Analysis: 1. Using the measured weight of the empty 125 mL weight when filled with water, and the known density of water at the temperature of the measurement, calculate the "effective" volume of the 125 mL Erlenmeyer flask, i.e., the volume available for occupancy by the H₂ gas. (You must also take into account the volume of the added HCl solution, which decreases the volume available to the H2 gas.) 2. Calculate the molar amounts of each piece of magnesium and unknown metal that you used. ENEW 3. Based on the measured temperatures and pressure changes for each reaction, use the ideal gas the molar amount of hydrogen gas that was produced in each reaction. 4. Calculate the volume occupied by one mole of hydrogen gas (molar volume) at STP. 5. Compare your calculated molar volume, at STP, with the accepted molar volume of an ideal gas at STP, viz., 22.41 L/mol. If the values do not compare well, suggest possible sources of experimental error. 6. Use your calculated value for the STP molar volume to determine the atomic weight of your unknown metal. What is the likely identity of the metal?

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Experiment 1 Mg Trial 1 Mass of Mg 0014 g Maximum pressur... View the full answer