rohopish
Feb 11, 2009, 03:46 PM
Hey y'all! I know this isn't a particularily stimulating discussion, but I've been working on this question for two days, it's driving me nuts, and I can't find an answer for it anywhere or even how to go about solving it.
For those who know some chemistry, the equilibrium constant equation is:
Keq = [products]/[reactants]
Now, I know how to find Keq, given the concentrations and number of moles of a reaction, but it's asking me to find the number of moles instead and says that Keq is equal to 3 during the reaction.
The "hint" given under the question says: "Let X be the number of
moles of each product formed at equilibrium. Substitute into the equilibrium equation using the moles of each reactant and product at equilibrium each divided by the total reaction volume. Leave the equilibrium concentrations as fractions. You can then take the square root of both sides of the equation after cancelling like terms, i.e. the volumes."
Could anyone help me with this? :confused: There must be some chem wizes on here.
Yours truly,
VERY FRAZZLED lol
For those who know some chemistry, the equilibrium constant equation is:
Keq = [products]/[reactants]
Now, I know how to find Keq, given the concentrations and number of moles of a reaction, but it's asking me to find the number of moles instead and says that Keq is equal to 3 during the reaction.
The "hint" given under the question says: "Let X be the number of
moles of each product formed at equilibrium. Substitute into the equilibrium equation using the moles of each reactant and product at equilibrium each divided by the total reaction volume. Leave the equilibrium concentrations as fractions. You can then take the square root of both sides of the equation after cancelling like terms, i.e. the volumes."
Could anyone help me with this? :confused: There must be some chem wizes on here.
Yours truly,
VERY FRAZZLED lol
