The reaction between MnO4− with C2O42− is as given below:
2MnO4−+16H++5C2O42−→2Mn+2+8H2O+10CO2
From this, we can see that 16 moles of H+react with 2 moles of MnO4− . Hence, one mole of permanganate requires eight moles of H+ ions
Number of moles of H+ ions required by 1 mole of MnO4− to oxidise oxalate ion to CO2 is ______.
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First and second ionization enthalpies of lithium are $520$ kJ mol$^{-1}$ and $7297$ kJ mol$^{-1}$ respectively. Energy required to convert $3.5$ mg lithium (g) into $\text{Li}^{2+}$(g) $[\text{Li(g)} \rightarrow \text{Li}^{2+}\text{(g)}]$ is _______ kJ mol$^{-1}$. (nearest integer) [Molar mass of Li $= 7$ g mol$^{-1}$]
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Work through every JEE Main Inorganic Chemistry PYQ, year by year.