For question 4, that value has to be greater than +23.56 not -23.56 because -50 is greater than -23.56 (speaking from a chemistry perspective not a mathematical one) note that enropy change is positive so if the enthalpy change is neagtive this must be a spontaneous reaction but if it is positive then it will be nonspontaneous at high temperatures which is the case here.
The values I used came from a standard reference booklet in the back of a textbook. We use Chemistry The Central Science (Brown LeMay), and it is in Appendix C of this textbook.
How did you arrive at that calculation? The given calculation looks correct. Entropy has been converted to kJ. The only way free energy could get larger is if entropy was negative, given exothermic reaction.
For question 4, that value has to be greater than +23.56 not -23.56 because -50 is greater than -23.56 (speaking from a chemistry perspective not a mathematical one) note that enropy change is positive so if the enthalpy change is neagtive this must be a spontaneous reaction but if it is positive then it will be nonspontaneous at high temperatures which is the case here.
Thank you sir for this awesome video 👍👍👍👍👍
The values I used came from a standard reference booklet in the back of a textbook. We use Chemistry The Central Science (Brown LeMay), and it is in Appendix C of this textbook.
Where did he get the values for the entropy??
From the table.basically u need one.they are constant value...
How we get the entropy?
Thank you sir
Good video.now i can score A.tq
For #2. c) shouldn't delta G=173kJ?
How did you arrive at that calculation?
The given calculation looks correct. Entropy has been converted to kJ. The only way free energy could get larger is if entropy was negative, given exothermic reaction.
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How you put values which is not given in a quetion
How
From the table he had
Thnxxxxx sir