For the reaction 2A+B=C+2D, the starting [A]=4.0M and [B]=3.0. At equilibrium the [C]=1.0M. Calculate the value of the equilibrium constant, K(c). I tried the formula but go no where because of "2D". Thank-you. a.)0.5 b.)2.0 c.)3.0 d.)3.5

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For the reaction 2A+B=C+2D, the starting [A]=4.0M and [B]=3.0. At equilibrium the [C]=1.0M. Calculate the value of the equilibrium constant, K(c). I tried the formula but go no where because of "2D". Thank-you. a.)0.5 b.)2.0 c.)3.0 d.)3.5

Chemistry
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Other answers:

you have to do an ICE table, are you familiar with that?
No I am not, i'm sorry.
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I= initial C= change E= equilibrium
Oh! yes, yes! but I am to given one. Only that statement.
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But how did you come up with those numbers?
Wait are those the coefficients?
So [1][2]/[2]^2[1]=.5?????
the problem said that you have at the equilibrium 1M of C. You have to assume that was 0 M of C at the beginning and 1 mole was produced. Then by the stoichiometry of the reaction you can calculate how much of A and B has to be consume to produce 1 mol of C.
no
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OMG thank-you!!!!! so simple.
@Cuanchi can I ask you another question?
sure if it fast
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I was trying to upload a picture of what I did as well xD
isolate the "x" that is just math
i got to go sorry
thank you so much!
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