the reaction is exothermic therefore the overall enthalpy change is negative -41.02. H1 should be -36.95 as it is an exothermic reaction as the temperature rose by 9. H2 is an endothermic reaction therefore should be +4.02.
Yes, I had the same doubt. Q = mcΔT however Q here is energy. Not ENTHALPY CHANGE. The equation for enthalpy change must be: ΔH=-mcΔT Hence ΔH3 in the experiment conducted would be -41.0 J per mole and not 41 J per mole. Correct me if I am wrong.
Hi, thank you for this video, it was really helpful. Can you please explain why after finding the temp change in Celsius you didn’t add 273 to convert it into kelvin? Because you changed the sign from c to k but the numbers remained the same.
Change in temperature is used in the equation so the difference in kelvin is same as difference in Celsius. Say temp changed from 20 to 25 C, 25 - 20 is same as (25+273) - (20+273)
This is really proof that not knowing something in this age is out of ignorance because there's so many resources on the internet that tach almost anything
@@theunknownchampion9492 alr thanks for the reply even though my exams ended a month ago lol, i realized it right after I sent the comment but didnt bother to remove it
i am so glad there's videos like this on the internet XD
the reaction is exothermic therefore the overall enthalpy change is negative -41.02. H1 should be -36.95 as it is an exothermic reaction as the temperature rose by 9. H2 is an endothermic reaction therefore should be +4.02.
Yes, I had the same doubt. Q = mcΔT however Q here is energy. Not ENTHALPY CHANGE. The equation for enthalpy change must be:
ΔH=-mcΔT
Hence ΔH3 in the experiment conducted would be -41.0 J per mole and not 41 J per mole.
Correct me if I am wrong.
@@pardhivkondreddy6848 wouldn't the equation for enthalpy change be (delta)H = -mc(delta)T/n ?
@@davankk2857 yes, if temp increases q=negative, if temp decreases q=positive, hence q is in J convert to KJ then Kj/Mol = enthalpy change
It's because it's supposed to be -q/n
Also delta H1 has been added up wrong, should be -37.62. Also, Delta H2 should be 4.01.
Many thanks Tabitha you're magic!
This is fantastic!
Love this. Thanks xx
I’m doing this practical next week, thank you for this video :-)
What grade did you get
wat grade did u get for ur final exam
Great vid ! 👍🏾
Can you please make videos on the other practicals as well as the a level ones
Thanks!
helped for my gcse next week
THANK YOUUU
Thank you
day before paper one
why are the arrows pointing down, i thought that was only used for combustion values?
mass of what? for the equation
thank you
im just confused why the arrows point downwards?
Hi, thank you for this video, it was really helpful. Can you please explain why after finding the temp change in Celsius you didn’t add 273 to convert it into kelvin? Because you changed the sign from c to k but the numbers remained the same.
Change in temperature is used in the equation so the difference in kelvin is same as difference in Celsius. Say temp changed from 20 to 25 C, 25 - 20 is same as (25+273) - (20+273)
i am curious as to how the anhydrous copper(ii)sulphate did not react with moisture in air to form hydrous copper(ii)sulphate?
I think it did a little bit because the colour is very slightly blue
This is really proof that not knowing something in this age is out of ignorance because there's so many resources on the internet that tach almost anything
shut the fuck up
yet still u cant spell 🤡🤡
I didn't understand the calculations
How did you get the 159.61 in 4.06/159.61?
This is the molar mass for cuso4 and she divided the mass by the molar mass so she gets moles
@@llii338 thank you
The units for Q are J not Jmol-1
Dear ma'am are these results accurate??
No.
everyone gets different results my friend. You are probably in university now so this probably will not help but just saying.
Is this applicable for CIE AS Level examinations?
check the specification on their website
why do we have to use 24cm^3 of water for the hydrated copper (II) sulfate but 25cm^3 of water for the anhydrous copper (II) sulfate?
because the hydrated copper already contains some water in it so to balance it out we use less of it. This may be a bit late lol
@@theunknownchampion9492 alr thanks for the reply even though my exams ended a month ago lol, i realized it right after I sent the comment but didnt bother to remove it
You forgot to minus the q. Everything else is helpful!
why didnt you convert the temp to kelvin?
you don't have to it is exactly the same my chem teacher said
5:28
didn't understand a word. :) thanks anyways
Ty 4 this girl I'm meant to write a method for this and it's due in 1 hour 😻😻😻