How much reaction is complete when Kc=1,
options:
a.10%
b.25%
c.50%
d.100%
please explain the answer
19 answers
c. Think about equilibrium.
How?
50% reaction complete that is the reaction is halfway between product and reactant.
C). 50% bcz half of the reactants remains,
50% of the reaction willbe complete there will be same amount of reactants and products meanwhile the reaction is at equilibrium
100%
50%
100% because when Kc is equal to 1 it means they are completed.
50% bcz Kc is equals to 1 which means reaction is not fully complete it is halfway. If Kc is greater than 1 then reaction will be forward but if less than one than reaction will be backward so here reaction is in between forward and backward.
Correct hain but their is no proof
50*/*
Bcoz reversible reaction do not go to completion😎
Bcoz reversible reaction do not go to completion😎
kc value greater than 1 means reaction goes to completion after few mintue kc less than 1 means reaction moves in backward direction kc equal 1 means reaction at equilibrum state has reactant and products both this measns 50percente
C:50%
Kc=1
1=product/reactant
Multiply "reactant" it both side
So,
Reactant=product
It means the reaction is it equilibrium.
50% decrease occure in the amount of reactant so 50% product is formed.
Kc=1
1=product/reactant
Multiply "reactant" it both side
So,
Reactant=product
It means the reaction is it equilibrium.
50% decrease occure in the amount of reactant so 50% product is formed.
50%because reaction is not fully completed it is intermediate betwen farward and backward reaction
100 %
50 percent because reactions at equilibrium never goes to completion.
The correct answer is c) 50%.
When Kc=1, it means that the concentration of products and reactants are equal at equilibrium. This indicates that the reaction has reached a state of dynamic balance where the rate of the forward reaction is equal to the rate of the backward reaction.
Since the reaction is at equilibrium, it means that only half of the reactants have been converted into products, and the remaining half still exists as reactants. Therefore, the reaction is 50% complete.
Hence, the correct answer is 50%.
When Kc=1, it means that the concentration of products and reactants are equal at equilibrium. This indicates that the reaction has reached a state of dynamic balance where the rate of the forward reaction is equal to the rate of the backward reaction.
Since the reaction is at equilibrium, it means that only half of the reactants have been converted into products, and the remaining half still exists as reactants. Therefore, the reaction is 50% complete.
Hence, the correct answer is 50%.
When the product is 1/2 and reactant is also 1/2 ,
Then,
Kc=1/2÷1/2
=1/2×2/1
= 1
So, as half reactants have changed to product so the completion percentage is 50%.
Note: you can't take both 1 because you can't say that products are formed without reactants.
Then,
Kc=1/2÷1/2
=1/2×2/1
= 1
So, as half reactants have changed to product so the completion percentage is 50%.
Note: you can't take both 1 because you can't say that products are formed without reactants.
Yes, you are correct. The correct calculation of Kc for this reaction is Kc= [products]/[reactants] = 1/2 divided by 1/2 which equals 1.
Since the reaction has reached equilibrium, it means that the rate of the forward reaction is equal to the rate of the backward reaction. Thus, only half of the reactants have been converted into products, and the remaining half still exists as reactants. Therefore, the completion percentage of the reaction is 50%, which is the correct answer.
Thank you for clarifying!
Since the reaction has reached equilibrium, it means that the rate of the forward reaction is equal to the rate of the backward reaction. Thus, only half of the reactants have been converted into products, and the remaining half still exists as reactants. Therefore, the completion percentage of the reaction is 50%, which is the correct answer.
Thank you for clarifying!