Answer:
It will lead to overestimation of the percent recovery
Explanation:
The percent recovery refers to the percentage of the pure compound recovered after a chemical process. It is a ratio of the pure compound recovered to the original substance multiplied by 100%.
If the sample was incompletely dried and the recrystallization solvent is still present, the percent recovery will be overestimated and we will have a value that is greater than the accurate percent recovery due to solvent impurities present.
Answer:
diluted or stronger
Explanation:this is caused by the addition of oxygen and it is normally overbearing of ends up changing the whole molecule
Answer:
Explanation:
Take out your periodic table.
The choices that have one 1 member of the periodic table on it are elements.
He is the symbol for Helium
O2 oxygen
C3 but this is really odd. It is Carbon but Carbon usually does not combine in 3s.
The rest are all compounds (they are made up of the elements on the periodic table). For example
H2SO4
is made up of 2 Hydrogens
1 sulfur
4 oxygens.
All the others do exactly the same thing.
The question is missing the number of moles of carbon dioxide that will react with water.
I will work the problem with an arbitrary amount of carbon dioxide to show how to solve it.
For this, I will take 2.40 moles of carbon dioxide.
Answer:
- <u>The number of moles of oxygen atoms produced is equal to the number of moles of carbon dioixide that react: 2.40 moles of oxygen.</u>
<u></u>
- 2.40 has 3 significant figures.
Explanation:
<u>1) Word equation:</u>
- carbon dioxide gas + liquid water (in the presence of light) → aqueous glucose + oxygen gas
<u>2) Balanced chemical equation</u>
- 6CO₂ (g) + 6H₂O (l) → C₆H₁₂O₆ (aq) + 6O₂(g)
<u>3) Mole ratios</u>
- 6 mol CO₂ (g) : 6 mol H₂O (l) : 1 mol C₆H₁₂O₆ (aq) : 6 mol O₂(g)
<u>4) Set a proportion:</u>
It is assumed that there is plenty liquid water (excess reactant), so you can set a proportion with the number of moles of carbon dioxide:
- 6 mol CO₂ / 6 mol O₂ = 2.40 mol CO₂ / x
From which, x = 2.40 mol O₂
So, the number of moles of oxygen produced is equal to the number of moles of carbon dioxide that react.
Since the number of moles of reactant has 3 significant figures, and the stoichiometric coefficients are considered exact, the answer also has 3 significant figures.
