QUESTION 4 65cm, what is the total pressue of the gas in the If the atmospheric

Question

QUESTION 4 65cm, what is the total pressue of the gas in the If the atmospheric pressure is 0.993 atm and the height of the wator column after the reaction occurs is 1 0.993 atm 0.991 atm 0 977 atm 0.971 atm QUESTION 5 20.5 C, what is the partial pressure of the hydrogen gas? t the total pressure of the gas in the eudiometer at the end of the experiment is 580.4mm Hg at 9598.6 mm Hg 31.89 mmig 0 105.6 mm Hg 582.2 mmig QUESTION 6 f the partial pressure of the hydrogen gas is 513.2 mmHg, the volume of the gas is 15.4 ml, and the temperature is 20.5 C, how many grams of hydrogen gas were formed? 0872 9 a72x 104 0.328 g 4.70g

Explanation / Answer

4. pressure of water column, PH2O= pressure of atm= 0.997atm

total pressure= PH2O + P H2

PH2= Pt-Ph20= 0.997-0.0313 = 0.971 atm { since pressure of H2O= 0.0313 atm}

5. Ptotal= PH2O + PH2

PH2= Ptotal - PH2O = 580.4 - 17.5 = 562.2 mmHg { since pressure of H2O= 17.5mmHg}

6. PtV=nRT

Pp H2= pressure= 513.2mmHg= (513.2*101.325)/760 = 68.42 kPa {since 760mmHg = 101.325 kPa}

PpH2O = 2.49kPa

Pt= 68.42+2.49= 70.91kPa

V= 15.4 ml= 0.0154 L

R= 8.314 JK-1mol-1

T= 20.5 oC= 293.5 K

put all the values in the formula, n= PV/RT = 0.000447 mol

n=mass/mol mass ,

mass of gas liberated = n*mol mass= 0.000447*2= 8.07 * 10-4 g.

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