Ok vs. Q
The principle distinction between (Ok) and (Q) is that (Ok) describes a response that’s at equilibrium, whereas (Q) describes a response that’s not at equilibrium. To find out (Q), the concentrations of the reactants and merchandise should be identified. For a given common chemical equation:
[aA + bB rightleftharpoons cC + dD tag{1}]
the Q equation is written by multiplying the actions (that are approximated by concentrations) for the species of the merchandise and dividing by the actions of the reactants. If any element within the response has a coefficient, indicated above with decrease case letters, the focus is raised to the ability of the coefficient. (Q) for the above equation is subsequently:
[Q_c = dfrac{[C]^c[D]^d}{[A]^a[B]^b} tag{2}]
A comparability of (Q) with (Ok) signifies which manner the response shifts and which aspect of the response is favored:
Exercise
One other vital idea that’s used within the calculation of the response quotient is named an exercise. For instance, think about the (Q) equation for this acid/base response:
[CH_3CH_2CO_2H{(aq)} + H_2O{(l)} leftrightharpoons H_3O^+{(aq)} + CH_3CH_2CO_2^-{(aq)} tag{3}]
The (Q) equation is written because the concentrations of the merchandise divided by the concentrations of the reactants, however solely together with elements within the gaseous or aqueous states and omitting pure liquid or strong states. The (Q) equation for this instance is the next:
[Q_c = dfrac{[H_3O^+{(aq)}][CH_3CH_2CO_2^-{(aq)}]}{[CH_3CH_2CO_2H{(aq)}]} tag{4}]
Outdoors Hyperlinks
References
Contributors and Attributions – “q calculator chemistry”