During the analysis, 0.163 g h2o and 0.600 g co2 are produced. calculate the amount (mol) h2o formed by combustion of 0.400 g vitamin c

Here we have to get the moles of water generated by the combustion of vitamin C.

4 moles of water (H₂O) will generate from the combustion of vitamin C.

The vitamin C is the ascorbic acid having the molecular formula C₆H₈O₆. On decomposition it produces water (H₂O) and carbon di oxide (CO₂).

The molecular weight of ascorbic acid is 176.12 g/mole.

In this analysis 0.163g of H₂O produces from 0.400g of vitamin C.

Thus from 176.12 g of vitamin C ×176.12 = 71.768 g of H₂O will produce.

The molecular weight of H₂O is 18 g/mole. Thus 71.768 g is equivalent to = 3.98 ≅ 4

Thus 1 mole of vitamin C (ascorbic acid) produces 4 moles of water on combustion.

The balanced combustion [in presence of excess oxygen (O₂)] reaction can be written as- C₆H₈O₆ + 5O₂ = 4H₂O + 6CO₂.

Thus the moles of water generated from combustion of vitamin C is determined.

"among the transition metal elements, manganese and zinc have a slight lowering of electronegativities. the reason behind this is that the nuclear charges of these elements are slightly weaker than the other transition metal elements due to the way their valence electrons are filled up. both manganese and zinc have their valence electrons filled up to the 4th shell with 1 pair of electrons (4s2) completely occupying it. although the electrons in the 3rd shell (3d) are yet to be paired since the outer most shell is filled up, the ability of the nucleus to attract electrons is lessened. hence,   the electronegativity (or the ability to attract electrons) is lessened."