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

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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

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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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