Calculate equilibrium constant?

In summary: So the problem is consistent.You have correctly calculated the equilibrium constant for the given reaction. However, the correct answer for the MCQ may be different due to rounding off or significant figures. It is possible that the correct answer is 11.7 when rounded off to one decimal place, even though the exact answer is 8.33. It is important to pay attention to the significant figures given in the question and use them in your calculations to get the closest possible answer.
  • #1
Aafia
70
1

Homework Statement


[/B]
The following reaction was allowed to reach the state of equilibrium
2A+B <====> C
The initial amounts of reactant present in one litre of solution were 0.5 mole of A and 0.6 mole of B. At equilibrium the amounts were 0.2 mole of A and 0.45 mole of B and 0.15 mole of C. Calculate equilibrium constant

Homework Equations



Kc= [product]/[reactants]

The Attempt at a Solution


[/B]
Kc= [0.15]/0.2^2×0.45
Kc=0.15/0.018
= 8.3
In my book one of the option of mcq given is 8.3 but the option marked as correct is 11.7 which one is right? If 11.7 is correct then how?
 
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  • #2
Aafia said:

Homework Statement


[/B]
The following reaction was allowed to reach the state of equilibrium
2A+B <====> C
The initial amounts of reactant present in one litre of solution were 0.5 mole of A and 0.6 mole of B. At equilibrium the amounts were 0.2 mole of A and 0.45 mole of B and 0.15 mole of C. Calculate equilibrium constant

Homework Equations



Kc= [product]/[reactants]

The Attempt at a Solution


[/B]
Kc= [0.15]/0.2^2×0.45
Kc=0.15/0.018
= 8.3
In my book one of the option of mcq given is 8.3 but the option marked as correct is 11.7 which one is right? If 11.7 is correct then how?

I do not see any reason your answer be wrong.

The question contains the superfluous information of initial concentrations, but as you can check these are consistent with the final.
 

Related to Calculate equilibrium constant?

1. What is an equilibrium constant?

An equilibrium constant (K) is a numerical value that represents the ratio of products to reactants at equilibrium in a chemical reaction. It is a measure of the extent to which a reaction proceeds to form products.

2. How is equilibrium constant calculated?

Equilibrium constant is calculated by taking the concentration of products and dividing it by the concentration of reactants, with each concentration raised to the power of its coefficient in the balanced chemical equation. The equation for equilibrium constant is K = [C]^c[D]^d / [A]^a[B]^b, where A, B, C, and D represent reactants and products, and a, b, c, and d represent their coefficients.

3. What is the significance of the equilibrium constant?

The equilibrium constant provides important information about a reaction, such as the direction in which it will proceed and the relative amounts of reactants and products at equilibrium. It also indicates the strength of the bond between reactants and products, with a higher K value representing a more stable equilibrium.

4. How does temperature affect the equilibrium constant?

The equilibrium constant is affected by temperature according to the Van 't Hoff equation, which states that K increases with increasing temperature for endothermic reactions and decreases for exothermic reactions. This is because temperature affects the equilibrium position of a reaction, with higher temperatures favoring the endothermic direction and lower temperatures favoring the exothermic direction.

5. Can the equilibrium constant be altered?

The equilibrium constant is a constant value at a given temperature, pressure, and concentration. It cannot be altered by changing these factors, but it can be altered by changing the reaction conditions, such as adding a catalyst or changing the volume of the reaction vessel.

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