Could you please find my mistake in this problem? I'm not getting the right answer. :[
Use the reactions below to predict the equilibrium constant for the reaction 2A(g)<->3D(g)
A(s)<->1/2B(g)+C(g) k1=0.0334
3D(g)<->B(g)+2C(g) k2=2.35
I know that you have to make modifications according to the stoichiometric coeffecients. So do I divide k1 by 2 and the multiply that by the inverse of 2.35 (which = 1/2.35 because the equation is reversed)?
I got this answer
0.0034/2=0.0167*(1/2.35)
=0.0071
sorry i did not mean to submit this question multiple times, my internet connection is low and i didn't think it went through. i apologize.
See my response to the original post.
To find the equilibrium constant for the reaction 2A(g) <-> 3D(g), you will need to use the given equilibrium constants (k1 and k2) for the reactions involving the substances A, B, and C.
First, let's analyze the stoichiometric coefficients of the two reactions to determine how they can be combined to obtain the desired reaction:
Reaction 1: A(s) <-> 1/2B(g) + C(g), k1 = 0.0334
Reaction 2: 3D(g) <-> B(g) + 2C(g), k2 = 2.35
To make necessary modifications, we consider the stoichiometric coefficients and account for the reverse reaction by taking the inverse of the corresponding equilibrium constant.
Step 1: Multiply reaction 1 by a factor of 2 to match the stoichiometry of A in reaction 2:
2A(s) <-> B(g) + 2C(g), k1' = (0.0334)^2 = 0.00111556
Step 2: Combine reaction 1 (multiplied by 2) and reaction 2 to obtain the desired reaction:
(2A(s) + 3D(g)) <-> (B(g) + 2C(g) + 2C(g)), k_combined = (k1')(1/k2) = (0.00111556)(1/2.35) = 0.000474901
Therefore, the equilibrium constant for the reaction 2A(g) <-> 3D(g) is approximately 0.000474901.
Based on your calculation, it seems you divided k1 by 2, which is correct. However, you didn't multiply it by the inverse of 2.35; instead, you multiplied it by 1 divided by 2.35. That is the main mistake in your calculation.
To correct it, divide k1 by 2 (which gives 0.0334/2 = 0.0167), then multiply it by the inverse of 2.35 (which gives 0.0167*(1/2.35) = 0.0071). Therefore, your revised answer should be 0.0071, not 0.0034.
I hope this explanation helps you understand how to find the equilibrium constant for a reaction by combining multiple reactions and making appropriate modifications to their equilibrium constants.