Hey can someone pls help me ASAP thanks!!!
1 answer:
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Answer:
C₁₀H₁₆O
Explanation:
Molecular formula can be determined from parent peak by using rule of thirteen.
Rule of Thirteen:
First divide the parent peak value by 13 as,
= 152 ÷ 13
= 11.69
Now, multiply 13 by 11,
= 13 × 11 (here, 11 specifies number of carbon atoms)
= 143
Now subtract 143 from 152,
= 152 - 143
= 9
Add 9 into 11,
= 9 + 11
= 20 (hydrogen atoms)
So, the rough formula we have is,
C₁₁H₂₀
Now, add one Oxygen atom to above formula and subtract one Carbon and 4 Hydrogen atoms as these numbers are equal to atomic mass of Oxygen atom as,
C₁₁H₂₀ -------O--------> C₁₀H₁₆O
Calculate Hydrogen deficiency index as,
HDI = (2x + 2 - y) / 2
where,
x = C atoms
y = H atoms
HDI = [2(10) + 2 - 16] / 2
HDI = (20 + 2 - 16) / 2
HDI = (22-16) / 2
HDI = 6 / 2
HDI = 3
It means, Camphor contains 1 double bond and two rings. As, HDI of double bond is 1 and HDI of one ring is 1.
(For a bit of context I will use the reaction between HCl and Mg as an example)
The larger the surface area of the magnesium metal, the more particles are exposed to collide with the aqueous HCl particles to cause the reaction to occur. This increases the frequency per second of collisions, speeding up the rate of reaction.
The effect of a catalyst is to reduce the minimum collision energy which allows the reaction to happen. This does not increase the number of collisions per second, but increases the percentage of successful collisions, which consequently causes the rate of reaction to increase .
I have drawn diagrams showing the effect of surface area, but there isn't really a meaningful diagram that I know of to show the impact of a catalyst (at least not at GCSE level).
The larger the surface area of the magnesium metal, the more particles are exposed to collide with the aqueous HCl particles to cause the reaction to occur. This increases the frequency per second of collisions, speeding up the rate of reaction.
The effect of a catalyst is to reduce the minimum collision energy which allows the reaction to happen. This does not increase the number of collisions per second, but increases the percentage of successful collisions, which consequently causes the rate of reaction to increase .
I have drawn diagrams showing the effect of surface area, but there isn't really a meaningful diagram that I know of to show the impact of a catalyst (at least not at GCSE level).