- #1
dRic2
Hi everybody,
Given a generic reaction ## Reagents ↔ Products ## the velocity of the reaction is ##R = R_{right} - R_{left} ##
To take in account that the velocity of the reaction will slow if approaching the equilibrium we say that
$$ R = R_{right}(1 - \frac K K_{eq}) $$
Although it seems reasonable it appears to me too much "arbitrary" so I don't get it very much. I mean, I could have elaborated an other relation to take the equilibrium into account or is it the only one?
Second question: A book of mine says that I reaction of first order such as ## A → B ## has
$$ R = kC_A(1- \frac K K_{eq} C_B) $$
but it seems wrong to me... Wouldn't it be
$$R = R_{right} - R_{left} = R_{right}(1 - \frac K K_{eq}) = kC_A(1- \frac K K_{eq} ) $$ ?
Given a generic reaction ## Reagents ↔ Products ## the velocity of the reaction is ##R = R_{right} - R_{left} ##
To take in account that the velocity of the reaction will slow if approaching the equilibrium we say that
$$ R = R_{right}(1 - \frac K K_{eq}) $$
Although it seems reasonable it appears to me too much "arbitrary" so I don't get it very much. I mean, I could have elaborated an other relation to take the equilibrium into account or is it the only one?
Second question: A book of mine says that I reaction of first order such as ## A → B ## has
$$ R = kC_A(1- \frac K K_{eq} C_B) $$
but it seems wrong to me... Wouldn't it be
$$R = R_{right} - R_{left} = R_{right}(1 - \frac K K_{eq}) = kC_A(1- \frac K K_{eq} ) $$ ?
Last edited by a moderator: