Write the correctly balanced net ionic equations for the reations whose equilibrium constant at 298 K are
` K_a (H_2C_2O_4)= 5.4 xx 10 ^(-2)`

Write the correctly balanced net ionic equations for the reations whose equilibrium constant at 298 K are K_b ( CH_3NH_2)= 4.4 xx 10^(-5)

Write the correctly balanced net ionic equations for the reations whose equilibrium constant at 298 K are K_a ( H_2S ) = 1.0 xx 10 ^(-7)

Write the correctly balanced net ionic equations for the reations whose equilibrium constant at 298 K are K_b( NH_3) = 1.8 xx 10 ^(-5)

Write a balanced equation for the C _(2) H _(4) + Br _(2) to

At a certain temperature , the following reactions have the equilibrium constants as shown below: S(s)+O_(2)(g)hArrSO_(2)(g),K_(c)=5xx10^(52) 2S(s)+3O_(2)(g)hArr2SO_(3)(g),K_(c)=10^(29) what is the equilibrium constant K_(c) for the reaction at tahea same temperature? 2SO_(2)(g)+O_(2)(g)hArr2SO_(3)(g)

Calculate equilibrium constant for the reaction CO+H_2O hArr CO_2+H_2 If equilibrium constants for 2CO+O_2hArr 2CO_2,K_1=40xx10^(-3) 2H_2+O_2hArr 2H_2O,K_2=36xx10^(-2)

Consider the following reaction. The reaction is first order in each direction, with an equilibrium constant of 10^(4) . For the conversion of chair form to boat form, e^(-Ea//RT)=4.35xx10^(-8) at 298 K with pre-exponential factor of 10^(12)s^(-1) . Apparent rate constant (k_(A)) at 298 K is :

Calculate the equilibrium constant (K) for the formation of NH^ in the following reaction: N_2(g) + 3H_2(g) At equilibrium, the concentration of NH_3 , H_2 and N_2 are 1.2 xx 10^(-2) ,3.0 xx 10^(-2) and 1.5 xx 10^(-2) M respectively.

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

For the reaction equilibrium, N_2O_4 (g) hArr 2NO_2 (g) the concentrations of N_2O_4 and NO_2 at equilibrium are 4.8 xx 10^(-2) and 1.2 xx 10 ^(-2) " mol " L^(-1) respectively . The value of K_c for the reaction is