Question

PbO2 oxidises MnO in presence of HNO3 the products are HMnO4 , Pb(nO3)2 and h2o calculate the number of moles of HNO3 and PbO2 consumed per mole of MnO?

Answer 1

You just balance the eqation

Answer 2

3 MnO + 5 PbO2 + 5 HNO3 = 3 HMnO4 + 5 Pb(NO3) + H2O
use this equation

Answer 3

the ans is 4 ,2

Answer 4

\[\begin{array}{cc} 5 \text{Pb}\text{O}_2 \\\end{array}+2MnO+10HNO_3 \rightarrow 2MnO_4+\begin{array}{cc} 5 \text{Pb}\left(\text{N}\text{O}_3\right)_2 \\ \end{array}+4H_2O\]

Answer 5

it is HMnO4

Answer 6

I mistake, but the balancing is correct

Answer 7

I've even checked with a software

Answer 8

the answer is 4,2 plzzz check it

Answer 9

calculate the number of moles of HNO3 and PbO2 consumed per mole of MnO?

Answer 10

If per mole of MnO then you have 5 moles of HNO3 and 2.5Moles of PbO2

Answer 11

you sure the reaction is correct?

Answer 12

yes

Answer 13

@.Sam. plzz help

Answer 14

calculate the number of moles of HNO3 and PbO2 consumed per mole of MnO? i think we have to do something here

Answer 15

The balancing is
\[\begin{array}{cc} 5 \text{Pb}\text{O}_2 \\\end{array}+2MnO+10HNO_3 \rightarrow 2HMnO_4+\begin{array}{cc} 5 \text{Pb}\left(\text{N}\text{O}_3\right)_2 \\ \end{array}+4H_2O\]

If per mole of MnO then you have 5 moles of HNO3 and 2.5Moles of PbO2, should be correct

Answer 16

you just divide 2 to all reactants and you get per mole of MnO

Answer 17

then you get per mole of MnO then 5 moles of HNO3 and 2.5Moles of PbO2

Answer 18

i think 4,2 is wrong answer.because when changing from MnO to HMnO4 Mn requires 5 electrons(since it changes from +2 to +7).each PbO2 will provide just 2 electrons.so 2 PbO2 will give only four electrons,which isn't sufficient.