The amount of water formed by combustion of 0.400 g vitamin C is .
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:
According to this reaction, one mole of reacts with five moles of and produce four moles of and six moles of . Therefore the stoichiometric ratio between and 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:
…… (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 .
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:
Learn more:
- Calculate the moles of chlorine in 8 moles of carbon tetrachloride: brainly.com/question/3064603
- 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.