| Assertion: If \[{{Q}_{c}}\](reaction quotient)\[<{{K}_{C}}\](equilibrium constant) reaction moves in direction of reactants. |
| Reason: Reaction quotient is defined in the same way as equilibrium constant at any stage of the reaction. |
| Read the assertion and reason carefully to mark the correct option out of the options given below: |
A) If both assertion and reason are true and the reason is the correct explanation of the assertion.
B) If both assertion and reason are true but reason is not the correct explanation of the assertion.
C) If assertion is true but reason is false.
D) If the assertion and reason both are false.
E) If assertion is false but reason is true.
Correct Answer: E
Solution :
[e] Assertion is false but reason is true. \[aA+bB\] ⇌\[cC+dD\], \[Qc=\frac{{{[C]}^{c}}{{[D]}^{d}}}{{{[A]}^{a}}{{[B]}^{b}}}\] If \[{{Q}_{c}}>{{K}_{c}}\], reaction will proceed in the direction of reactants. If \[{{Q}_{c}}<{{K}_{c}}\], reaction will move in direction of products. If \[{{Q}_{c}}={{K}_{c}}\], the reaction mixture is already at equilibrium.
You need to login to perform this action.
You will be redirected in
3 sec
