For the equilibrium
`N_(2)+3H_(2) hArr 2NH_(3)` at 298K
and 5 atm. Pressure, increasing pressure to 50 atm, will ( here K is the equilibrium constant )

For the equilibrium H_(2) O (1) hArr H_(2) O (g) at 1 atm 298 K

For the equilibrium H_(2) O (1) hArr H_(2) O (g) at 1 atm 298 K

On decomposition of NH_(4)HS , the following equilibrium is estabilished: NH_(4) HS(s)hArrNH_(3)(g) + H_(2)S(g) If the total pressure is P atm, then the equilibrium constant K_(p) is equal to

On decomposition of NH_(4)HS , the following equilibrium is estabilished: NH_(4) HS(s)hArrNH_(3)(g) + H_(2)S(g) If the total pressure is P atm, then the equilibrium constant K_(p) is equal to

The equilibrium constant for the reversible reaction N_(2)+3H_(2) hArr 2NH_(3) is K and for the reaction (1)/(2) N_(2)+(3)/(2) H_(2) hArr NH_(3) , the equilibrium constant is K',.K and K' will be related as

For the equilibrium of the reaction NH_(4) Cl(s) hArr NH_(3) (g) + HCl (g) Kp = 81 atm^(2) . Total pressure at equilibrium will be x times the pressure of NH_(3) . The value of x will be ........

What is the effect of increasing pressure on the equilibrium N_2 +3H_2hArr 2NH_3 ?

For the following reaction : NH_(2) COO NH_(4) (s) hArr 2 NH_(3) (g) + CO_(2) (g) If the total pressure of the system at equilibrium is 3 atm , then the value of K_(p) will be -