`6 xx 10^(-3)` mole `K_2 Cr_2 O_7` reacts completely with `9 xx 10^(-3)` mole `X^(n+)` to given `XO_3^- and Cr_^(3+)`. The value of `n` is :

6xx10^(-3) mole K_(2)Cr_(2) C_(7) reacts completely with 9xx10^(-3) mole X^(n+) to give XO_(3)^(-) and Cr^(3+) . The value of n is :

How many moles of K_2Cr_2O_7 required to react completely with 1 mol of H_2S in acidic medium?

1.0 mole of Fe reacts completely with 0.65 mole of O_(2) to give a mixture of only FeO and Fe_(2)O_(3) the mole ratio of ferrous oxide to ferric oxide is

For 1.34xx10^(-3) moles of KBrO_3 to reduce into bromide 4.02 xx 10^(-3) mole of X^(n+) ion is needed. New oxidation state of X is:

An element A in a compound ABD has oxidation number A^(n-) . It is oxidised by Cr_(2)O_(7)^(2-) in acid medium. In the experiment 1.68xx10^(-3) moles of K_(2)Cr_(2)O_(7) were used for 3.26xx10^(-3) moles of ABD . The new oxidation number of A after oxidation is:

A 2.18 g sample contains a mixture of XO and X_(2)O_(3) . It reacts with 0.015 moles of K_(2)Cr_(2)O_(7) to oxidize the sample completely to form XO_(4)^(-) " and " Cr^(3+) . If 0.0187 mole of XO_(4)^(-) is formed , what is the atomic mass of X ?

6 mole of FeC_2 O_4 on treatment with 2 mole of K_2 Cr_2 O_7 in acidic medium evolves x litre of CO_2 gas at STP. The value of x would be:

A solution containing 2.7 xx 10^-3 mol of A^(2+) irons required 1.6 xx 10^(-3) mole of MnO_4^- for the oxidation of A^(2+) to AO_3^- the medium used is :

2.68xx10^(-3) moles of solution containing anion A^(n+) require 1.61xx10^(-3) moles of MnO_(4)^(-) for oxidation of A^(n+) to AO_(3)^(-) in acidic medium. What is the value of n ?

2.68xx10^(-3) moles of solution containing anion A^(n+) require 1.61xx10^(-3) moles of MnO_(4)^(-) for oxidation of A^(n+) to AO_(3)^(-) in acidic medium. What is the value of n ?