A mixture of one mole of CO_(2) and one mole of H_(2) attains equilibrium at a temperature of 250^(@)C and a total pressure of 0.1 atm for the change CO_(2(g)) +H_(2(g)) harr CO_((g))+H_(2)O_((g)). Calculate K_(P) if the analysis of final reaction mixture shows 0.16 volume fraction of CO

A mixture of one mole of CO_(2) and one mole of H_(2) attains equilibr

1.	A mixture of one mole of CO_(2) and one mole of H_(2) attains equilibrium at a temperature of 250^(@)C and a total pressure of 0.1 atm for the change CO_(2(g)) +H_(2(g)) harr CO_((g))+H_(2)O_((g)). Calculate K_(P) if the analysis of final reaction mixture shows 0.16 volume fraction of CO
Answer» <P>0.46 0.63 0.22 0.82 Solution : volume FRACTION = pressure fraction = mole fraction `X_(CO)=X_(H_(2)O)=0.16` `X_(CO_(2))=X_(H_(2))=(1-2 XX 0.16)/(2)=0.34` `K_(P)=((X_(CO) xx P)(X_(H_(2)O) xx P))/((X_(CO_(2)) xx P)(X_(H_(2)O) xx P))` `=(0.16 xx 0.16)/(0.34 xx 0.34)=0.22`