Trial 1 Trial 2 Measured Data Mass of Mg (g) Volume of H2 gas (mL) (4pts) 4o. 2O

Question

Trial 1 Trial 2 Measured Data Mass of Mg (g) Volume of H2 gas (mL) (4pts) 4o. 2Oml Barometric Pressure (mm Hg) (2pts) (2pts) .035 0.01 41LmL (i.e., Atmospheric Pressure) Temperature (oC) (3pts) 21"l Calculations: Moles of Mg reacted (4pts) Show Calculations: (2) no Calculation (show work) (Note: Not calculated from molarity of HCl): (4pts) mok of mg released /1 mole of H2 Vapor Pressure of water from Figure 1 in mmHg (2pts) 8.TmmtH Pressure of H2 from Dalton's Law in mmHg (4pts) 22.3mn Show Calculations: (4pts) 410 1g 22.3mmtg 34

Explanation / Answer

Pressure of H2 in atm = 722.3 mmHg x 1atm/760mmHg

= 0.9504 atm

Gas constant R for trial 1

From the ideal gas equation

Volume of H2 gas = 40.20 mL x 1L/1000mL = 0.04020 L

PV = nRT

R = PV/nT

= (0.9504 atm x 0.04020 L)/(0.00146 mol x 294.15K)

= 0.088963 L-atm/mol-K

Gas constant R for trial 2

From the ideal gas equation

Volume of H2 gas = 41.20 mL x 1L/1000mL = 0.04120 L

PV = nRT

R = PV/nT

= (0.9504 atm x 0.04120 L)/(0.00171 mol x 294.15K)

= 0.077846 L-atm/mol-K

Average R = (0.077846 + 0.088963)/2

= 0.083404 L-atm/mol-K

% error = ( 0.083404 - 0.08206)*100/0.08206

= 1.64%

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