Answer : The equilibrium concentration of
at
is,
.
Solution : Given,
Equilibrium constant, 
Initial concentration of
= 0.260 m
Let, the 'x' mol/L of
are formed and at same time 'x' mol/L of
are also formed.
The equilibrium reaction is,

Initially 0.260 m 0 0
At equilibrium (0.260 - x) x x
The expression for equilibrium constant for a given reaction is,
![K_c=\frac{[H_3O^+][C_2H_3O_2^-]}{[HC_2H_3O_2]}](https://tex.z-dn.net/?f=K_c%3D%5Cfrac%7B%5BH_3O%5E%2B%5D%5BC_2H_3O_2%5E-%5D%7D%7B%5BHC_2H_3O_2%5D%7D)
Now put all the given values in this expression, we get

By rearranging the terms, we get the value of 'x'.

Therefore, the equilibrium concentration of
at
is,
.
Answer:
periods
Explanation:
Know the periodic table
- Hope that helped! Let me know if you need a further explanation.
<u>Answer:</u> The value of equilibrium constant for reverse reaction is 
<u>Explanation:</u>
The given chemical equation follows:

The equilibrium constant for the above equation is 
We need to calculate the equilibrium constant for the reverse equation of above chemical equation, which is:

The equilibrium constant for the reverse reaction will be the reciprocal of the initial reaction.
If the equation is multiplied by a factor of '
', the equilibrium constant of the reverse reaction will be the 1/2 power of the equilibrium constant of initial reaction.
The value of equilibrium constant for reverse reaction is:

Hence, the value of equilibrium constant for reverse reaction is 
I think the correct answer from the choices listed above is the second option. A way that the elements are grouped on the periodic table would be that elements with similar bonding properties are in the same column. <span>Each column is called a </span>group<span>. The elements in each </span>group<span> have the same number of electrons in the outer orbital.</span>