desired Mg mass =0.0340g  "Atmospheric pressure (mmHg): 733.59 Trial 1 and Trial 2 values separated by commas: Mass of Mg (g): 0.038, 0.031 Temperature (°C): 20.2 (both trials) Vapor pressure of water (mmHg): 17.86 (both trials) Volume of gas (mL): 42.95, 35.80 need calculations for table.

(a) Mass of Magnesium metal used (b) Volume of H₂ gas collected (c) Temperature of H₂ gas collected (d) Atmospheric Pressure (e) Temperature of Water in bath (bucket) (f) Vapor Pressure of Water at above temperature Volume of H₂ gas (in L) Temperature of H2 gas (in K) Moles of H₂ gas Pressure of H₂ gas (in atm) Experimental value of R (include units) Average value of R (include units): Trial 1 0.043 g 44.00 mL Percent Error between your average value and the theoretical value of R (show work): 22.5 °C 765 mm Hg 21.0 °C 18.7 mm Hg Using your experimental data, determine the value of R, the gas constant. Show all your conversions and calculations for each step clearly in the table below. Pay attention to units and significant figures. Trial 1 Trial 2 Trial 2 0.042 g 42.00 mL 22.0 °C 769 mm Hg 22.0 °C 19.3 mm Hg

Solve like the example attached.  Apply the significant figure rule to your final answer.

For a gaseous sample, Pressure (P) and quantity (n) are inversely related directly related No answer text provided. O No answer text provided.