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You don't have to apply the Hess Cycle if you don't see the necessityI don’t understand why we have to do Hess law, what’s its importance any way if we can just do the subtraction method
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You don't have to apply the Hess Cycle if you don't see the necessityI don’t understand why we have to do Hess law, what’s its importance any way if we can just do the subtraction method
View attachment 65243Can someone explain this question to me please?
Thank you , appreciate It
View attachment 65246 Help please
I would go for option A because if you write the formulas they result in the same reaction i.e burning carbon results in Only Carbon dioxide under standard Conditions.Moreover it relates to standard Conditions and hence we can trust that it gives the standard enthalpy of formation of CO2View attachment 65246 Help please
I would go for option A because if you write the formulas they result in the same reaction i.e burning carbon results in Only Carbon dioxide under standard Conditions.Moreover it relates to standard Conditions and hence we can trust that it gives the standard enthalpy of formation of CO2
B is wrong for me because bond energies are based on averages and are not entirely standard e.g compare the C and O double bond in acetone,ethanal and carbon dioxide ... They will vary because of the environments the carbon is in .
C is wrong because the combustion of carbon may not necessarily be at standard conditions and hence the enthalpy change of reaction will not necessarily give the standard enthalpy of formation of carbon dioxide
D is wrong because the enthalpy change of combustion from Diamond is non standard
I believe A is the correct answer for those reasons what do you think ?
[/QUO
I was stu
i was stuck in between A and B , well I guess I’ll rely on your answer because I’m a novice to ASI would go for option A because if you write the formulas they result in the same reaction i.e burning carbon results in Only Carbon dioxide under standard Conditions.Moreover it relates to standard Conditions and hence we can trust that it gives the standard enthalpy of formation of CO2
B is wrong for me because bond energies are based on averages and are not entirely standard e.g compare the C and O double bond in acetone,ethanal and carbon dioxide ... They will vary because of the environments the carbon is in .
C is wrong because the combustion of carbon may not necessarily be at standard conditions and hence the enthalpy change of reaction will not necessarily give the standard enthalpy of formation of carbon dioxide
D is wrong because the enthalpy change of combustion from Diamond is non standard
I believe A is the correct answer for those reasons what do you think ?
I am also doing AS 😁
In Sodium HydrideThe oxidation number of H is +1, but it is -1 in when combined with less electronegative elements.
what examples are there that makes hydrogen more electronegative hence giving it a negative -1 ?
In Sodium Hydride
And how does the box diagram look like for elements beyond potassium , how do we fill it diagrammaticallyHello again, there’s a question that’s rather bothering . Can someone just explain why is it the “b” optionView attachment 65252
Oxidation states (oxidation numbers)
Explains what oxidation states (oxidation numbers) are, and how to calculate them and make use of them.www.chemguide.co.uk
We use what is called the Hund's rule to fill up the atomic orbitals. Electrons fill up lower energy levels before they can fill higher ones. In this case we have 1st,2nd and 3rd energy levels . So electrons will fill up 1 then 2 then 3 in that order.Hello again, there’s a question that’s rather bothering . Can someone just explain why is it the “b” optionView attachment 65252
There will be introduction of the d orbitals which will be tedious to explain here. But the same principles of orbital filling apply . I will post a link to a YouTube videoAnd how does the box diagram look like for elements beyond potassium , how do we fill it diagrammatically
There will be introduction of the d orbitals which will be tedious to explain here. But the same principles of orbital filling apply . I will post a link to a YouTube video
There will be introduction of the d orbitals which will be tedious to explain here. But the same principles of orbital filling apply . I will post a link to a YouTube video
We are one another's strength 💯💯Thank you so much for clearing my doubts😄
Indeed👍🏻We are one another's strength 💯💯
You are welcome 😊
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