One third litre of x M K_2Cr_2O_7 is requir | vedclass

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Question

(B) The balanced chemical equation for the reaction is: $Cr_2O_7^{2-} + 6Fe^{2+} + 14H^+ \longrightarrow 2Cr^{3+} + 6Fe^{3+} + 7H_2O$ Moles of ferrous

Vedclass · Accepted Answer

$0.1$

Vedclass · Answer

(B) The balanced chemical equation for the reaction is: $Cr_2O_7^{2-} + 6Fe^{2+} + 14H^+ \longrightarrow 2Cr^{3+} + 6Fe^{3+} + 7H_2O$ Moles of ferrous ammonium sulphate $= M 	imes V = 0.1 \ M 	imes 2 \ L = 0.2 \ mol$. From the stoichiometry, $1 \ mole$ of $K_2Cr_2O_7$ reacts with $6 \ moles$ of $Fe^{2+}$. Moles of $K_2Cr_2O_7$ required $= \frac{0.2}{6} = \frac{0.1}{3} \ mol$. Molarity $x = \frac{n}{V} = \frac{0.1/3 \ mol}{1/3 \ L} = 0.1 \ M$. Thus, option $(B)$ is correct.

One third litre of $x \ M \ K_2Cr_2O_7$ is required to completely oxidise $2 \ L$ of $0.1 \ M$ ferrous ammonium sulphate in acidic medium. What is $x$?

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