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Department
Chemistry
Course Code
CHM135H1
Professor
Kris Quinlan

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EXAM: 3 hours; 5 short answers, 28 M/C questions
-half of exam is new material (untested)
-other half is units 1 to 4
LECTURE 14
Slide No. Notes
-electrochemistry deals with relationship between chemical
reactions and electricity
-spontaneous reactions can produce electricity and electricity can
cause non-spontaneous reactions to occur
1-Delta S is negative because entropy of gas greater than that of
liquids
-Spontaneity – calculate delta G
-H and O gas both 0
-Therefore spontaneous
-Delta G = Delta H etc. formula
-Both delta H and delta S are negative
-Whenever both signs the same, some temperatures spontaneous
some not
-Reaction becomes non-spontaneous at high temperatures
-To calculate K for the reaction…
-Delta G = -RTInK
-Q = 1/ (P of H2)squared times P of O2 = 1
-Therefore K is greater than one for reaction to go to products
-Therefore answer either E or D
-To actually determine K
-(1000J/kJ)(-474kJ) = (-8.314J/molK)(298K)InK
-K = 1.44x10^83 therefore reaction goes to completion
-Ans: E
-To calculate temperature when reaction non-spontaneous
-Calculate temperature when reaction switches from non-
spontaneous to spontaneous
-Delta G = Delta H – T times delta S with delta G = 0
-Delta H = 2mol(-285.8kJ/mol) = -571.6kJ
-Delta S = 2mol(699.9J/molK) – 2mol(130.6J/molK)
1mol(205J/molK) = -326.4J/K
-T = delta H/delta S = 1751 K
-Reaction is non-spontaneous at temperatures above 1751K
2-LEO: losing electrons is oxidation; GER: gaining electrons is
reduction
-OIL RIG
-overall reaction – electrons cancel out
-
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Description
EXAM: 3 hours; 5 short answers, 28 MC questions - half of exam is new material (untested) - other half is units 1 to 4 LECTURE 14 Slide No. Notes - electrochemistry deals with relationship between chemical reactions and electricity - spontaneous reactions can produce electricity and electricity can cause non-spontaneous reactions to occur 1 - Delta S is negative because entropy of gas greater than that of liquids - Spontaneity calculate delta G - H and O gas both 0 - Therefore spontaneous - Delta G = Delta H etc. formula - Both delta H and delta S are negative - Whenever both signs the same, some temperatures spontaneous some not - Reaction becomes non-spontaneous at high temperatures - To calculate K for the reaction - Delta G = -RTInK - Q = 1 (P of H2)squared times P of O2 = 1 - Therefore K is greater than one for reaction to go to products - Therefore answer either E or D - To actually determine K - (1000JkJ)(-474kJ) = (-8.314JmolK)(298K)InK - K = 1.44x10^83 therefore reaction goes to completion - Ans: E - To calculate temperature when reaction non-spontaneous - Calculate temperature when reaction switches from non- spontaneous to spontaneous - Delta G = Delta H T times delta S with delta G = 0 - Delta H = 2mol(-285.8kJmol) = -571.6kJ - Delta S = 2mol(699.9JmolK) 2mol(130.6JmolK) 1mol(205JmolK) = -326.4JK - T = delta Hdelta S = 1751 K - Reaction is non-spontaneous at temperatures above 1751K 2 - LEO: losing electrons is oxidation; GER: gaining electrons is reduction - OIL RIG - overall reaction electrons cancel out - www.notesolution.com
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