i am talking about the 65th question, in the below given uploaded photo, i.e. the first order decomposition curves

enter image description here

as per the given reaction for every mole of A3 decomposed, there is a liberation of 3/2 moles of A2 but when their concentration becomes equal, then the system is at equilibrium so. but how can i calculate the amount of reactant that has been decomposed


Let initial concentration be C of $\small A_3$ then after some times let it decrease by D, so $\small A_2$'s concentration increase by $3/2$ $\times$ D because of stoichiometric ratios, when equal $\small C-D=(3/2)D$ so $\small D=(2/5)C$. So concentration of $A_3$ reduced by $2/5$th or $40\%$.

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