Watch a video of the procedure by clicking here. From the video you will need to record the following data: Volume of H, gas collected in mL: 42.95 mL Height of the water column in cm: 9.3 cm Temperature of water in °C: 23,2 °C Perform the following calculations: 1. Using the balanced chemical equation below, determine the moles of hydrogen gas produced when 0.0408 g Mg reacts. Mg + 2HC1 → MgCl, + H2 2. Convert the height of the water column to the pressure of the water column in mm Hg using the equation below (cm water)x10 13.6 %3D water 3. Determine the pressure of the hydrogen gas if the air pressure was 751.5 mmHg. PH, = P air – P %3D waer 4. Convert the pressure of hydrogen gas from mmHg to atmospheres. mmHg 760 atm = 5. Convert the temperature from Celceus to Kelvin. 6. Determine the volume of hydrogen gas in L 7. Use the ideal gas law, PV = nRT, to determine the value of the R. 8. Based on a value of 0.0821 Latm/molK, determine the percent error for this experiment. experimental value of R-0.0821 0.0821 x 100 Percent Error %D

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