Question

8. H2 and O2 is mixed and then placed in a 5.00 L. flask at 22 °C. The H2 partial pressure is 2.7 atm and the O2 partial pressure is 1.5 atm. What is the mole fraction of H2? (3 points)

Answer 1

8) total volume is V = 5.00 L

T = 295K

The partial pressure of an individual gas is equal to the total pressure multiplied by the mole fraction of that gas.

Ptotal = PH2 + PO2 = 2.7 + 1.5 = 4.2 atm

Assuming both gases are acting as an ideal gas, PV = nRT and

P = (nRT) / V

PH2 = xH2 * Ptotal

Mole fraction of H2 = xH2 = PH2 / Ptotal = 2.7 * / 4.2 = 0.643

Equilibrium constant expression:

a ) SbCl5(g) <--------> SbCl3(g) + Cl2(g)

Keq = {[SbCl3] [Cl2]} / [SbCl5]

b ) 2BrNO <----------> 2NO + Br2

Keq = [NO]^2[Br2] / [BrNO]^2

c ) CH4 +2H2S <---------> CS2 + 4H2

Keq = [CS2][H2]^2 / [CH4][H2O]^2

d ) 2CO + O2 <----------> 2CO2

Keq = [CO2]^2 / [CO]^2 [O2]