Question

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

Answer 1

The amount of water formed by combustion of 0.400 g vitamin C is $\boxed{0.00908{\text{ mol}}}$.

Further Explanation:

To determine:

Amount of water formed during combustion of 0.400 g of vitamin C.

How to proceed:

Step I: First of all, balanced chemical reaction for combustion reaction of vitamin C is written.

Balanced chemical reaction for combustion of vitamin C is as follows:

 ${{\text{C}}_6}{{\text{H}}_8}{{\text{O}}_6} + 5{{\text{O}}_2} \to 4{{\text{H}}_{\text{2}}}{\text{O}} + 6{\text{C}}{{\text{O}}_2}$

According to this reaction, one mole of ${{\text{C}}_{\text{6}}}{{\text{H}}_{\text{8}}}{{\text{O}}_{\text{6}}}$ reacts with five moles of ${{\text{O}}_{\text{2}}}$  and produce four moles of ${{\text{H}}_{\text{2}}}{\text{O}}$ and six moles of ${\text{C}}{{\text{O}}_{\text{2}}}$. Therefore the stoichiometric ratio between ${{\text{C}}_{\text{6}}}{{\text{H}}_{\text{8}}}{{\text{O}}_{\text{6}}}$ and ${{\text{H}}_{\text{2}}}{\text{O}}$ is 1:4

Step II: Moles of vitamin C present in 0.400 g are to be determined. This can be done with the help of equation (1).

The formula to calculate moles of component is as follows:

${\text{Moles of component}} = \dfrac{{{\text{Mass of component}}}}{{{\text{Molar mass of component}}}}$                                          …… (1)

Substitute 0.400 g for mass of component and 176.12 g/mol for molar mass of component in equation (1) to calculate moles of ${{\text{C}}_{\text{6}}}{{\text{H}}_{\text{8}}}{{\text{O}}_{\text{6}}}$.

$\begin{aligned} {\text{Moles of }}{{\text{C}}_{\text{6}}}{{\text{H}}_{\text{8}}}{{\text{O}}_{\text{6}}} &= \frac{{{\text{0}}{\text{.400 g}}}}{{{\text{176}}{\text{.12 g/mol}}}} \\ &= 0.00227{\text{ mol}} \\ \end{aligned}$  

Since one mole of vitamin C forms four moles of water, number of moles of water formed by 0.00227 moles of vitamin Ccan be calculated as follows:

$\begin{aligned} {\text{Moles of }}{{\text{H}}_{\text{2}}}{\text{O}} &= \left( {{\text{0}}{\text{.00227 mol }}{{\text{C}}_{\text{6}}}{{\text{H}}_{\text{8}}}{{\text{O}}_{\text{6}}}} \right)\left( {\frac{{{\text{4 mol }}{{\text{H}}_{\text{2}}}{\text{O}}}}{{{\text{1 mol }}{{\text{C}}_{\text{6}}}{{\text{H}}_{\text{8}}}{{\text{O}}_{\text{6}}}}}} \right) \\ &= 0.00908{\text{ mol}} \\ \end{aligned}$  

Learn more:

1. Calculate the moles of chlorine in 8 moles of carbon tetrachloride: brainly.com/question/3064603
2. Calculate the moles of ions in the solution: brainly.com/question/5950133

Answer details:

Grade: Senior School

Subject: Chemistry

Chapter: Mole concept

Keywords: H2O, 0.00908 mol, vitamin C, H2O, CO2, O2, 5O2, C6H8O6, four moles, 0.00227 mol, 4 mol, 1 mol.

Answer 2

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 $\frac{0.163}{0.400}$×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 $\frac{71.768}{18}$ = 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.