Asked by kenzie
2 C6H6 + 15 O2 → 12 CO2 + 6 H2O ΔHrxn = 6542 kJ/rxn
If 8.88 g of C6H6 (FW = 78.114 g/mol) is burned and the heat produced from the reaction is used to heat 6354 g of water at 22.5o C, what is the final temperature of the water (swater = 4.184 J/g C)? (Write answer to 1 place past the decimal point)
If 8.88 g of C6H6 (FW = 78.114 g/mol) is burned and the heat produced from the reaction is used to heat 6354 g of water at 22.5o C, what is the final temperature of the water (swater = 4.184 J/g C)? (Write answer to 1 place past the decimal point)
Answers
Answered by
bobpursley
two moles of benzene yield 6542kJ
so how many moles do you have? Ans 8.88/78.14
so the heat produced is 6542*(8.88/(2*78.14) kJ=371kj
heat produced=masswater*c*(Tf-22.5) solve for Tf
I get about a 14C rise in temp. Watch units, kj,kg,g
so how many moles do you have? Ans 8.88/78.14
so the heat produced is 6542*(8.88/(2*78.14) kJ=371kj
heat produced=masswater*c*(Tf-22.5) solve for Tf
I get about a 14C rise in temp. Watch units, kj,kg,g
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.