Help with these questions Atmospheric pressureMass of magnesium metalVolume of 6 M hydrochloric acidVolume of molecular hydrogen gasData TableUse the following table to record your data for each trial.Water temperaturePartial pressure of water (at abovetemperature)Name:CalculationsDo the following calculations for each trial.MacyTrial 1Trial 20.9939am0.0779 0.0709 0.080g8.4mL 8.8mL80.01 ml21.0c0.9939a0.9939atmTrial 38.1ML76.02m 72.01mL21.1 c21.2 c18.765 torr 18.880118.880kom 18.650-0.9939atm1atm755.4mmlly• 760mmigforr2Pressure 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.9939 P-2Moles 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). 116 |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.m

Given, Reaction of magnesium metal with HCI .

Data Table Use the following table to record your data for each trial. 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 1 Trial 2 Trial 3 0.9939a0.9939am 0.9939atm 0.0779 0.0709 0.080g 8.4mL 8.8mL 18.1mL 76.02m 72.01mL 80.01ml 21.1'c 21.2°C 21.0c 18.765 tor 18.880kom 18.650 torr 755.4mmHg. -=0.9939atm 1atm 760mmHg 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 adix 3) calculate the pressure of molecular hydrogen gas for each trial.

Data Table Use the following table to record your data for each trial. 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 1 Trial 2 Trial 3 0.9939a0.9939am 0.9939atm 0.0779 0.0709 0.080g 8.4mL 8.8mL 18.1mL 76.02m 72.01mL 80.01ml 21.1'c 21.2°C 21.0c 18.765 tor 18.880kom 18.650 torr 755.4mmHg. -=0.9939atm 1atm 760mmHg 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 adix 3) calculate the pressure of molecular hydrogen gas for each trial.

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter15: Solutions

Section: Chapter Questions

Problem 10CR

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