Chemical Forums
Chemistry Forums for Students => High School Chemistry Forum => Topic started by: collinryans on February 21, 2010, 12:11:08 PM
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Hi, I am having trouble with this question. Could someone tell me how to do it, I'm not sure what I am doing is right or not so it would help to see other peoples answers.
The question is:
The equilibrium constant for the reaction represented below is 50 at 4480C.
H2(g) + I2(g) ::equil:: 2HI(g)
a) How many moles of HI are present at equilibrium when 1.0 moles of H2 is mixed with 1.0 moles of I2 in a 0.50 L Container and allowed to react at 4480C?
b) How many moles of H2 and I2 are left unreacted?
c) If the conversion of H2 and I2 to HI is essentially complete, how many moles of HI would be present?
d) What is the percent yield of the equilibrium mixture?
for a) I got 7, I'm not even sure how to do the other ones.
Thanks in advance.
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[H2]=[I2] = 1/0,5=2 and K=[HI]^2 /[H2][I2]=50
at the equilibrium;
[HI]= X
[H2]= 2-x
[I2] = 2-x
now pleace these above equation
50=x^2/(2-x)^
I think you can do after this