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There are 11 Carbon atoms in the compound.
<u>Solution:</u>
Carbon atom count is the ratio of the M peak to the M+1 peak.
![\text{ Number of Carbon atoms }=\frac{\text { Relative intensity of } M+1 \text { peak }}{0.011 \times \text { Relative tntensity of } M \text { peak }}](https://tex.z-dn.net/?f=%5Ctext%7B%20Number%20of%20Carbon%20atoms%20%7D%3D%5Cfrac%7B%5Ctext%20%7B%20Relative%20intensity%20of%20%7D%20M%2B1%20%5Ctext%20%7B%20peak%20%7D%7D%7B0.011%20%5Ctimes%20%5Ctext%20%7B%20Relative%20tntensity%20of%20%7D%20M%20%5Ctext%20%7B%20peak%20%7D%7D)
Here M peak is 57.10% and M+1 peak is 6.83%. On applying the values in the formula we get,
![\frac{0.0683}{0.011\times0.571g} = 10.87\approx11](https://tex.z-dn.net/?f=%5Cfrac%7B0.0683%7D%7B0.011%5Ctimes0.571g%7D%20%3D%2010.87%5Capprox11)
Therefore, the number of Carbon atoms in the compound are 11.
Refer the image attached below for a better understanding of M peak and M+1 peak.
The heaviest ion that has the greatest m/z value is said to be the molecular ion peak in mass spectrum.
Answer:
Both Arrhenius Base and Bronsted Lowry Base
Both Arrhenius Acid and Bronsted Lowry Acid
Arrhenius Acid Only
Arrhenius Base Only
Bronsted Lowry Acid Only
Bronsted Lowry Base Only
Explanation:
Answer:
Vapor pressure of solution = 23.9 Torr
Explanation:
Let's apply the colligative poperty of vapor pressure to solve this:
ΔP = P° . Xm
ΔP = Vapor pressure of pure solvent - Vapor pressure of solution
We have solvent and solute mass, so let's find out the moles of each.
55.3 g / 62 g/mol = 0.89 moles
285.2 g / 18 g/mol = 15.84 moles
Let's determine the mole fraction of ethylene glycol.
Mole fraction = Moles of ethylene glyco / Total moles
0.89 moles / (0.89 + 15.84) = 0.053
25.3 Torr - Vapor pressure of solution = 25.3 Torr . 0.053
Vapor pressure of solution = 25.3 Torr . 0.053 - 25.3 Torr
Vapor pressure of solution = 23.9 Torr
Answer:
1552.83J Released
Explanation:
1. mass/m=225
Initial temp:86C, final:32.5C
Changed Temp: 32.5-86= -53.5C
s=0.129 J/gC
Formula: q= m times s times changed Temp.
q=(225)(0.129)(-53.5)
q= -1552.83 J
q=1552.83 J Released