Answer : The volume of 
produced at standard conditions of temperature and pressure is 0.2422 L
Explanation :
Combined gas law is the combination of Boyle's law, Charles's law and Gay-Lussac's law.
The combined gas equation is,
where,
= initial pressure of 
gas = (740-22.4) torr = 717.6 torr
= final pressure of gas at STP= 760 torr
= initial volume of gas = 280 mL
= final volume of gas at STP = ?
= initial temperature of gas = 
= final temperature of gas = 
Now put all the given values in the above equation, we get:
Therefore, the volume of produced at standard conditions of temperature and pressure is 0.2422 L
Answer:
2.05mg Fe/ g sample
Explanation:
In all chemical extractions you lose analyte. Recovery standards are a way to know how many analyte you lose.
In the problem you recover 3.5mg Fe / 1.0101g sample: <em>3.465mg Fe / g sample. </em>As real concentration of the standard is 4.0 mg / g of sample the percent of recovery extraction is:
3.465 / 4×100 = <em>86,6%</em>
As the recovery of your sample was 1.7mg Fe / 0.9582g, the Iron present in your sample is:
1.7mg Fe / 0.9582g sample× (100/86.6) = <em>2.05mg Fe / g sample</em>
<em></em>
I hope it helps!
A because if you multiple it, you will be moving the decimal one time
There are three possible Isomers for Molecular Formula C₃H₄. Isomers are;
1) Propyne 2) Propa-1,2-diene 3) CyclopropeneStructures of all three isomers are given below.
There are no geometrical isomers for given molecular formula because geometrical isomers are formed in compounds containing double bond with at least two bulky groups at both sp² hybridized carbons. In given isomers, propyne does not contain any double bond, Propa-1,2-diene is symmetrical in nature while cyclopropene is a 3-membered ring. And for cycloalkenes there must be other groups attached to ring other than Hydrogen atom, hence cyclopropene does not contain any other group, so it can not show geometrical isomerism.
Answer:
Air is made up of 78.09% nitrogen, 20.95% oxygen, 0.93% argon, 0.04% carbon dioxide, and other gases in meager amounts.
