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Ajay Sabarish
Ajay Sabarish
11:11
sir i have a major doubt in chemical equilbrium can you please clear it?
say we have a reaction N2O4 ---\ 2NO2
\----

for this reaction,if initial number of moles of N2O4 is 'a' can we write

t = 0 a -
at equilbrium a-x 2x

similarly can we do the same for pressure i.e.
if initial pressure is p,then can we say

t=0 p -
at equilbrium p-y 2y

if yes why? and is x=y,i.e is the number of moles x dissociated equal to decrease in pressure of reactant?
and is this method valid for all reversible reaction irrespective of the stoichiometric coefficient of reactants and products
 
5 hours later…
Brian
Brian
15:55
@AjaySabarish If you post something new here, make sure to start the first message with "@Brian". That way I get a notification.
I'm having a little trouble understanding your equations
the formatting is kind of unclear
but if you have a mixture of gases that are "ideal" in their behavior, then in a constant-volume container and at constant temperature, the pressure and the total number of moles of gas are strictly proportional
see:
Ideal gas law
The ideal gas law is the equation of state of a hypothetical ideal gas. It is a good approximation to the behavior of many gases under many conditions, although it has several limitations. It was first stated by Émile Clapeyron in 1834 as a combination of Boyle's law, Charles' law and Avogadro's Law. The ideal gas law is often written as: where: P is the pressure of the gas V is the volume of the gas n is the amount of substance of gas (in moles) R is the ideal, or universal, gas constant, equal to the product of the Boltzmann constant and the Avogadro constant. T is the temperature of the gas...
P = (RT/V) * n
Many gases behave this way, especially at lower total pressures
so, "is this method valid for all reversible reaction irrespective of the stoichiometric coefficient of reactants and products?"
Answer: Yes, as long as all of the gases exhibit ideal gas behavior.

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