Help Data TableUse the following table to record your data for each trial.Trial 1Atmospheric pressureMass of magnesium metalVolume of 6 M hydrochloric acidVolume of molecular hydrogen gasName: Macy HuffordWater temperaturePartial pressure of water (at abovetemperature)CalculationsDo the following calculations for each trial.Trial 219.0c16.48tomTrial 329.39inH29.39in29.39in0.085g 0.0779 0.0839110.0mL 10.0m 10.00L86.63mL77.50ml 79.60019.0c19.0cPressure of H, gas: Assume that water and molecular hydrogen are the only gases inside the tube.Using the measured atmospheric pressure and the partial pressure of water vapor (determined fromthe temperature - see Appendix 3), calculate the pressure of molecular hydrogen gas for each trial.Trial 1: Patm=29,39inHgx254cmx10mm-746.506mmHg1inMoles of H,gas: Using the molar mass of magnesium and the balanced equation for the reactionyou have just observed, calculate the moles of molecular hydrogen that should have been formed.This calculation assumes that the magnesium was pure and was completely consumed by thehydrochloric acid, and that no H₂ was lost in the process (i.e., it assumes a 100% yield of hydrogengas). San Diego Miramar College | Chem 152L LaboratoryCalculations (continued)Use the ideal gas law, the pressure of H, and moles of H, calculated above, along with the volumeand temperature from your data table, to calculate the ideal gas constant (R) for each trial.Calculate the average value of R for your three trials.Calculate the % error between your average and the literature value of R = 0.08206 L-atm/K mol.

The given reaction, Mg+2HCl → MgCl2+H2 Given that, Atmospheric pressure = 29.39 in Hg (all the three…

Data Table Use the following table to record your data for each trial. Trial 1 Atmospheric pressure Mass of magnesium metal Volume of 6 M hydrochloric acid Volume of molecular hydrogen gas Water temperature Partial pressure of water (at above temperature) Calculations Do the following calculations for each trial. Trial 2 19.0c 16.48tor Trial 3 29.39in29.39in29.39in 0.085g 0.0779 0.08.39 10.0mL 10.0m 10.0mL 86.63mL77.50ml 79.60m 19.0c 19.0°c Pressure of H, gas: Assume that water and molecular hydrogen are the only gases inside the tube. Using the measured atmospheric pressure and the partial pressure of water vapor (determined from the temperature - see Appendix 3), calculate the pressure of molecular hydrogen gas for each trial. Trial 1: Patm = 29.39inHgx254cmx10mm=746.506mmHg Moles of H,gas: Using the molar mass of magnesium and the balanced equation for the reaction you have just observed, calculate the moles of molecular hydrogen that should have been formed. This calculation assumes that the magnesium was pure and was completely consumed by the hydrochloric acid, and that no H, was lost in the process (i.e., it assumes a 100% yield of hydrogen gas).