An unopened soda has an aqueous concentration of `CO_(2)`at`25^@`equal to `0.0408`molal.Thus ,pressure of `CO_(2)`gas in the can is `(K_(H)=0.034 mol//kg ba r)`

Molality of an aqueous solution that produce an elevation of boiling point of 1.00 K at 1 atm pressure. K_(b) for water is 0.512 K kg mol^(-1)

A 10L flask at 300K contains a gaseous mixture of CO and CO_(2) at a total pressure of 2.0 atm. If 0.2 mol of CO is present, the partial pressure of CO_(2) is ( Use R = 0.082 atm mol^(-1) K^(-1) )

1.0 molal aqueous solution of an electrolyte X_(3)Y_(2) is 25% ionized. The Boiling point of the solution is (K_(b) of H_(2)O=0.52K kg mol^(-1))

1.0 molal aqueous solution of an electrolyte X_(3)Y_(2) is 25% Ionised. The boiling point in the solutioin is ( K_(b) for H_(2)O=0.52K kg mol)

The freezing point of an aqueous solution of non-electrolyte having an osmotic pressure of 2.0 atm at 300 K will be, (K_(f) "for " H_(2)O = 1.86K mol^(-1)g) and R = 0.0821 litre atm K^(-1) mol^(-1) . Assume molarity and molality to be same :

Calculate the ratio of pressure of CO_(2)" gas and "CO gas at equilibrium in the reaction, CO_(2) (g)+C(s) Leftrightarrow 2CO(g) , If K_(p) is 3 bar at 900K and initial pressure of CO_(2) is 0.48 bar.

Molality of an aqueous solution that produces an elevation of boiling point of 1.00K at 1 atm pressure (K_(b) for water =0.512K.kg." mol"^(-1))

1.0 molal aqueous solution of an electrolyte X_(3)Y_(2) is 25% ionised . The boiling point of the solution is : ( K_(b) for H_(2)O = 0.52K kg/mol)