# chemistry

For the equilibrium H2(g)+CO2(g)<-->H2O(g)+CO(g)
Kc=3.18 at 1106 K.If each of the four species was initially present at a concentration of 3.000M,Calculate the equilibrium concentration of the CO (g) at this temperature.
Choices 0.844
3.268
3.844
3.460
2.156
Thanks anyone that can help

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3. 👁 361
1. Here is how you do a problem like this.
Prepare an ICE chart.

initial:
H2 = 3.000
CO2 = 3.000
H2O = 3.000
CO = 3.000

Next we must determine which way the reaction will go. So you set up the reaction quotient.
Qc = (3.000)(3.000)/(3.000)(3.000) = 1.000
Now compare Qc with Kc. Q<Kc ( 1 vs 3.18) and that means the products are too small and the reactants are too large. (You get that from the fraction).That means the reaction will be going to the right to reach equilibrium. Now complete the ICE chart.

change:
H2O = +x
CO = +x
CO2 = -x
H2 = -x

equilibrium (final):
H2O = 3.000-x
CO = 3.000-xx
H2 = 3.000+x
CO2 = 3.000+x

Substitute the equilibrium numbers into the Kc expression and solve for x. Then add 3.000 or subract x from 3.000 to arrive at the individual concn.

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posted by DrBob222
2. DR bob
I got that far no probs...But don't know how to do the last bit could you expand please
Thanks andy

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posted by Andy
3. Your note isn't clear. Did you solve for x and obtain a number. If not, here is the equation. Solve for x. If you have a value of x, see below.
Kc = 3.18 = (3.000+x)(3.000+x)/(3.000-x)(3.000-x)
Solve for x.

I don't know what x is because I didn't solve the equation; however, let me just make up a number for x. Let's say it is 0.01.
Then CO = 3.000 + 0.01 = ??
H2O = 3.000 + 0.01 = ??
CO2 = 3.000 - 0.01 = ??
H2 = 3.000 - 0.01 = ??

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posted by DrBob222
4. DR Bob,
If I plug in 0.01 for x then the answer is (3.000+0.01)times(3.000+0.01)divided by (3.000-0.01)times(3.000-0.01)answer according to my calculator says 9.0601.....ok how does that relate to the answer??am I to keep guessing what X isuntill I get the answer? or is there an easy way to get x?? sorry if seem a bit vague but I don't know where to go from here...
Andy....thanx for your help so far I am starting to get it......

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posted by Andy
5. No. Why choose 0.01. You solve the equation. You don't guess. Leaving off the zeros, the equation is
(3+x)(3+x)/(3-x)(3-x) = 3.18
This actually is
(3+x)^2/(3-x)^2 = 3.18
Now take the the square root of both sides.
(3+x)/(3-x) = sqrt(3.18)
Now solve for x

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6. Dr BOB,
How this
(3+0.844)^2/(3-0.844)^2=3.18(rounded)
sqrt(3.18)=1.7832
So there fore answer=0.844 which is one of the answers!
Am I on the right track?
Andy

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posted by Andy
7. Yes and no.
Yes, that's the value of x. No, that isn't the right answer. I thought you could do the problem since I worked 99.9% of it. But not so. Apparently you guessed enough times to find the right answer of 0.844 for x and that is correct. But you didn't need to spend all that time guessing. Such a waste of time, too.
(3.000+x)^2/(3.000-x)^2 = 3.18
Take the square root of both sides.
(3.000+x)/(3.000-x) = 1.78326
3.000+x = 1.78326(3.000-x)
3.000+x = 5.34977 - 1.78326x
x+1.78326x = 5.34977-3.000
2.78326x = 2.34977
x = 2.34977/2.78326
x = 0.8442 which I would round to 0.844 M and I didn't need to guess at the answer. But that isn't the anwer to the problem. The question asks for (CO) at equilibrium. If you will look at the ICE chart set up, we let 3.000+x = (CO); therefore, 3.000 + 0.844 = 3.844M for (CO).

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8. Thanks Dr Bob,
I am horrible at algebra....
But since reading your reasoning I have now got ammunition to be able to reason out the answer....I will try harder and study more..
Thanks for all your advice it was great
Andy

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posted by Andy

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