Initially 3 moles of 'A' was taken in a 1 L container. The approx. moles of A left in the container when the following equilibrium estblished is `x xx 10^(-6)`. The value of 'x' is
`3A hArr B, K_(C)=8xx10^(15)`

For are reaction Ato product, initially 10 mole of A is taken. In 80 minutes 9.375 mole of A is found to be reacted. The rate constant of the reaction is represented as 3.5xx10^(-x)"min"^(-1) . What is the value of X

In 5 litre container 1 mole of H_(2) and 1 mole of I_(2) are taken initially and at equilibrium of HI is 40% . Then K_(p) will be

In 5 litre container 1 mole of H_(2) and 1 mole of I_(2) are taken initially and at equilibrium of HI is 40% . Then K_(p) will be

The value of DeltaG^(@) for a reaction is 7.97 KJ//"mole" . Its equilibrium constant K_(c) at 298K is 4 xx 10^(-x) What is x?

PCl_(5) hArr PCl_(3) + Cl_(3) " "K_(c)= 1.844 3.0 moles of PCl_(5) is introduced in a 1 L closed reaction vessel at 380 K. The number of moles of PCl_(5) at equilibrium is ________ xx 10^(-3) . (Round off to the Nearest Integer)

Calculate the pH of a buffer solution containing 0.1 mole of acetic acid and 0.15 mole of sodium acetate. K_(c) for acetic acid is 1.75 xx 10^(-5) .

A(g)hArr B(g)+C(g),K_C=10^(-8) C(g)hArr D(g),K_C=10^(-5) 1 mole of A(g) is taken in a closed container of volume 1 litre at temperature T. If concentration of D at equilibrium is 10^(-x) , then , calculate value of x.

3 mole of reactant A and one mole of reactant B are mixed in a vessel of volume 1 litre . The reaction taking place is A + B hArr 2 C . If 1.5 mol of C is formed at equilibrium , the value of K_(c) is