`PCl_(5)(g)` density (in g/L) of mixture at 24 atm and `300 K`, when `PCl_(5)(g)` undergo `50 %` decomposition. `[R = 0.08 "atm L mol"^(-1) K^(-1)]`

Density of ideal gas at 2.46 atm and 300 K is 0.8 g//L Hence g-molar mass of gas is : [R = 0.082 "L-atm/mol-K"]

Calculate percentage change in M_(avg) of the mixture, if PCl_(5) undergo 50% decomposition. PCl_(5) rArr PCl_(3) + Cl_(2)

For the reaction : PCl_(3)(g)+Cl_(2)(g)hArr PCl_(5)(g) the value of K_(c ) at 250^(@)C is 26. The value of K_(p) at this temperature will be : (R = 0.082 L atm mol^(-1)K^(-1) )

What is the molar mass of a gas whose density is 1.5 g L^(-1) at 27^(@)C and 1 atm pressure ? (Use R = 0.08L atm mol^(-1) K^(-1) )

For a 5% solution of urea (Molar mass - 60 g/mol), calculate the osmotic pressure at 300 K. [R = 0.0821 L atm K^(-1) mol^(-1)]

For a 5% solution of urea (Molar mass - 60 g/mol), calculate the osmotic pressure at 300 K. [R = 0.0821 L atm K^(-1) mol^(-1)]

PCl _(5) (g) to PCl _(3) (g) + Cl _(2) (g) In the above first order reaction the concentration of PCl _(5) reduces from initial concentration 50 mol L ^(-1) to 10 mol L ^(-1) m 120 minutes at 300K. The rate constant for the reaction at 300 K is x xx 10 ^(-2) "min"^(-1). The value of x is ______________[Given log 5 = 0.69989 ]