Exp 3 (Intro) DATA AND REPORT * Show Name Section # SECTION DATE PARTNER your wo

Question

Exp 3 (Intro) DATA AND REPORT * Show Name Section # SECTION DATE PARTNER your work and keep track of significant figures Daa A. Mass of muagnesium rilblon Temperature of the Water Barometric Pressure B. C. -2196 inchHg (fram CRC Handhboolo.... 23.6 mmilg 22ml Vapor Pressure of Water (from CRC Handbool) E. Volume of gas in gas collection tube Calculations 1. Change unit total pressure in collection tube (mmHg) 2. Pressure of dry gas (in atm) 3. Amount of hydrogen gas (in moles) 4. Temperature of gas (in Kelvin) 5. Volume of hydrogen gas (in liters) 6. Experimental value of R 7 %Error

Explanation / Answer

total pressure = 29.96 inches of Hg, 29.92 inches of Hg= 1 atm

29.96 inchrs of Hg= 29.96/29.92 atm=1 atm, vapor pressure of water= 23.06 mm Hg= 23.06 mm Hg* 1atm/760 mm Hg= 0.0303, partial pressure of dry gas= total pressure- saturation pressure of water= 1-0.0303 =0.9697 atm

P= 0.9697 atm, V= 32.1ml= 32.1/1000 L= 0.0321L ( 1000ml=1L), T= 24.5 deg.c= 24.5+273= 297.5 K

The reaction is Mg+2HCl ------->MgCl2+ H2, 1 mole of Mg gives rise to 1 mole of H2

moles of Mg= mass/atomic weight =0.0321/24 =0.00134

moles of H2=0.00134, R= gas law constant= PV/nT =0.9697*0.0321/(0.00134*297.5)=0.0781 L.atm/mole.K

% error= 100*{(0.0821-0.0781)/0.0821}=4.9%

Actual value of R= 0.0821 L.atm/mole.K

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