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.