Home
Class 12
CHEMISTRY
At a certain temperature, equilibrium co...

At a certain temperature, equilibrium constant `(K_(c))` is 16 for the reaction,
`SO_(2)(g)+NO_(2)(g)hArrSO_(3)(g)+NO_(g)`
If we take one mole each of all the four gases in a one litre container, what would be the equilibrium concentrations of `NO` and `NO_(2)`?

Text Solution

Verified by Experts

The correct Answer is:
NA
Promotional Banner

Topper's Solved these Questions

  • CHEMICAL AND IONIC EQUILIBRIUM

    IIT-JEE PREVIOUS YEAR (CHEMISTRY)|Exercise OBJECTIVE_TYPE|3 Videos

  • CHEMICAL AND IONIC EQUILIBRIUM

    IIT-JEE PREVIOUS YEAR (CHEMISTRY)|Exercise COMPREHENSION_TYPE|3 Videos

  • CARBOXYLIC ACID AND THEIR DERIVATIVES

    IIT-JEE PREVIOUS YEAR (CHEMISTRY)|Exercise CHAPTER TEST|3 Videos

  • CHEMICAL BONDING

    IIT-JEE PREVIOUS YEAR (CHEMISTRY)|Exercise MATCH THE COLUMN|1 Videos

Similar Questions

Explore conceptually related problems

At a certain temperature, equilibrium constant (Kc) is 16 for the reaction, SO_(2)(g) + NO_(2)(g) rarr SO_(3)(g) + NO(g) If we take one mole each of all the four gases in a one litre container, what would be the equilibrium concentrations of NO "and" NO_(2) ?

At a certain temperature, equilibrium constant (K_(c)) is 16 for the reaction: SO_(2)(g)+NO_(2)(g) hArr SO_(3)(g)+NO(g) If we take 1 mol of each of the four gases in a 1-L container, what would be the equilibrium concentrations of NO and NO_(2) ?

At a certain temperature the equilibrium constant K_(c) is 0.25 for the reaction A_(2)(g)+B_(2)(g)hArrC_(2)(g)+D_(2)(g) If we take 1 mole of each of the four gases in a 10 litre container ,what would be equilibrium concentration of A_(2) (g)?

At a certain temperature the equilibrium constant K_(c) is 0.25 for the reaction A_(2)(g)+B_(2)(g) hArr C_(2)(g)+D_(2)(g) If we take 1 mole of each of the four gases in a 10 litre container, what would be equlibrium concentration of A_(2)(g) ?

At a certain temperature , the equilibrium constant (K_(c)) is 4//9 for the reaction : CO(g)+H_(2)O(g) hArr CO_(2)(g)+H_(2)(g) If we take 10 mole of each of the four gases in a one - litre container, what would be the equilibrium mole percent of H_(2)(g) ?

At a certain temperature, the equilibrium constant (K_(c )) is 16 for the reaction: SO_(2)(g)+NO_(2)(g)hArrSO_(3)(g)+NO(g) If we take one mole of each of the equilibrium concentration of NO and NO_(2) ?