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
