If `Ag + 2NH_3 iff [Ag(NH_3)_2]`
`K_1 = 1.8 xx 10^7`
`Ag^+ +Cl^- iff AgCl`
`K_2 = 5.6 xx 10^9`
Then for `AgCl + 2NH_3 iff [Ag(NH_3)_2]^+ + Cl^-`
What will be the value of equilibrium constant?

If Ag^(+)+2NH_3iff[Ag(NH_3)_2]^(+) K_1=1.8xx10^7 Ag^(+)+Cl^(-)iffAgCl K_2=5.6xx10^9 Then for AgCl+2NH_3iff[Ag(NH_3)_2]^(+)+Cl^- What will be value of equilibrium constant?

Give the IUPAC name of the complex: [Ag(NH_3)_2]Cl .

The following concentrations were obtained for the formation of NH_3 from N_2 and H_2 at equilibrium at 500K. [N_2] = 1.5 xx 10^-2M. [H_2] = 3.0 xx10^-2 M and [NH_3] =1.2 xx 10^-2 M . Calculate equilibrium constant.

For the reaction, 2NH_3(g) iff N_2(g) + 3H_2(g) the units of K_p will be

What is the IUPAC name of [Ni(NH_(3))_(6)]Cl_(2) ?

Oxidation state of Cr in [Cr(NH_3)_4Cl_2]^+

For the reversible reaction N_2(g)+3H_2(g) iff 2NH_3(g) +heat The equilibrium shifts in forward direction

This question has Statement I and Statement II. Of the four choices given after the Statements, choose the one that best describes the two Statements Statement - I : If equilibrium constant for N_2 + 3H_2 iff 2 NH_3 is K, the equilibrium constant for 1/2N_2+3/2 H_2 iff NH_3 will be K/2 Statement II: On dividing or multiplying an equation with any number, the equilibrium constant of the reaction changes