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chiu152_aut07_q4_key

# chiu152_aut07_q4_key - Name kg E Section TA Quiz#4 Useful...

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Unformatted text preview: Name: kg E] Section: TA: Quiz #4 Useful Constants: Faraday’ s Constant - 96, 485 C/mol; h (Planck’s constant)= 6. 63 x 10 34 J s; c (Speed of light): 3 x 108 m s ;N (Avogadro’ 3 number): 6. 022 x 1023 mol';l' R= 8. 314 J/mol. K Useful Equations: AG° = —nFE°ce11; AG° = -RT1n(K); E°ce11 = (0.0257 V / n) ln(K); AG = -nFEce11 ; AG = AG° + RTln(Q); Been = 13°C.,“ - (0.0591 V/n)log(Q) (1) (3 pt) The equilibrium constant for the reaction 2Hg(l) + 2Cl_(aq) + Ni2+(aq) —) Ni(s) + Hg2C12(s) is 5.6 x 10~20 at 25°C. Calculate the value of E° for a cell utilizing this reaction. @ZM.\\\\OC\U¥W; .7 Ecdl‘O On& Q— ——\< ' ., n? +1 a; [0: za- 0 (Pg-£41.03 (K0 ”7%(K K» :0 “0971950: 0.0%: 23092: é”: O 05“ Ce Carlo ) r 0‘0qu (461 235;) «Cl *umsﬁ “ti ‘l- o 42.3 . ...:.[ 5 =~o. 57 v1 (2) (2 pts) What 15 E for the half-reaction below 2H (aq, 1.00 M) + 2c ~—> H2(g, 1.00 atm) xii) S fancim‘ck )r\ (Sq?) ef\ @\e,d(®<&e, (3) (3 pt) Calculate E for the half-reaction below at 25°C. 2H (aq, 1.00 x 10‘5 M) + 2e* —> H2(g, 1.00 atm) __ ﬂ " Q 1 9+ :1?) 5_ ”Eva OSQlLﬂ’Q C12.) (:13 ‘5 “0.40. 58qu :0“ 0 0:“ £030 acme”) 0.056(1 :~ 2 (lo) 03(le (2) (a) (3 pt) Balance the redox reaction corresponding to the following electrochemical cell: N 0 {Nag} Zn*2[Zn anodle. (,OVVAOAL The Standard reduction potential for the N204 l N03 half cell 18 0. 83V. The Standard reduction potential for the an I Zn half cell 18- 0. 76V. ho\§(7‘h5 “but“ _ ‘ _ (”31¢ N20“! ”VA/03 +5» b ’11?" .32 + 2c»; azn 0» our; nms 149* Fae“: :cdamocjlﬂ“ Once/QC - -O.76V «0 .83V [email protected]] +39% K :waZH 0.:sq1.\ in It 2 ...
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