For the equilibrium system
`2HX(g) hArr H_(2)(g)+X_(2)(g)`
the equilibrium constant is `1.0xx10^(-5)`. What is the concentration of HX if the equilibrium concentration of `H_(2)` and `X_(2)` are `1.2xx10^(-3)` M, and `1.2xx10^(-4)` M respectively?

For the equilibrium system 2HX(g) hArr H_(2)(g)+X_(2)(g) the equilibrium constant is 1.0xx 10^(-5) . What is the equilibrium concentration of HX if the equilibrium concentrations of H_(2) and X_(2) are 1.2xx10^(-3) M and 1.2 xx 10^(-4) M respectively ?

For the equilibrium system : 2HCl(g)hArr H_(2)(g)+Cl_(2)(g) the equilibrium constant is 1.0xx10^(-5) . What is the concentration of HCl if the equilibrium concentration of H_(2) and Cl_(2) are 1.2xx10^(-3) M and 1.2xx10^(-4) M respectively ?

For the reaction, 2HCl_((g))hArrH_(2(g))+Cl_(2(g)) , the equilibrium constant is 1.0xx10^(-5) . What is the concentration of HCl if the equilibrium concentrations of H_(2) and Cl_(2) are 1.2xx10^(-8)M and 1.2xx10^(-9)M respectively?

For the equilibrium 2SO_(3(g))hArrSO_(2(g))+O_(2(g)) , the value of equilibrium constant is 4.8xx10^(-3) at 700^(@)C . At equilibrium, if the concentration of SO_(3) and SO_(2) are 0.60M and 0.15M respectively. Calculate the concentration of O_(2) in the equillibrium mixture.

For the equilibrium 2SO_(3(g))hArrSO_(2(g))+O_(2(g)) , the value of equilibrium constant is 4.8xx10^(-3) at 700^(@)C . At equilibrium, if the concentration of SO_(3) and SO_(2) are 0.60M and 0.15M respectively. Calculate the concentration of O_(2) in the equillibrium mixture.

For the equilibrium 2SO_(3(g))hArrSO_(2(g))+O_(2(g)) , the value of equilibrium constant is 4.8xx10^(-3) at 700^(@)C . At equilibrium, if the concentration of SO_(3) and SO_(2) are 0.60M and 0.15M respectively. Calculate the concentration of O_(2) in the equillibrium mixture.

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.

Calculate the equilibrium constant (Kc) for the formation of NH_(3) in the following reactions. N_(2)(g) +3H_(2)(g) hArr 2NH_(3)(g) At equilibrium, the concentration of NH_(3), H_(2) and N_(2) are 1.2 xx 10^(-2), 3.0xx10^(-2) and 1.5xx10^(-2) respectivley.