chem kinetics worksheet

8/12/2019 Chem Kinetics worksheet

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bleclrorlsrs ot r\aur )u'""-' *''' "':" ::-ilg ot"opp". ru* a.po.ited in a copper voltameter ;n series with theelectr,rlltic cell. Durrng the rame Ierlo0 1 I ^-

of gases liberated at STP will be:(A) 12.+ ml (B) I 12 ml (C) 168 ml (D) 336 mlOn electrolysing KrSOi solution tlsing inerl electrodes' l-68 L (STP) ofgases was obtained Horv many moles ofMnO; could be red,rced ro Mnr* by the same quantity ofelectriciq - --(A) o.r0 (B) 0.20 (c) 0.r 5 rD) 0.02\.\ hai cLrrreni sr.ngth \oulti be reqLrrred io pfoduce l)]drogen gas at thc rate oi I 12 cin'sr (STP) bj the"i""""iv'i. "r"q*.*

lacl solution \riih 96 570 : T:"i:T'i*:I: " , " ^(A) 0.65 A (B) 9.31 A (c) 10.00 A (D) 0.10 AThe pli oi0.5 L of 1.0 M NaCI after the electrol)'tl: 1"^':I5 t "ils:;o-* current ( 100% efficiencv)' is:(A) r.00 (B) r 3.00 (c) 12.70 (D) r.30Electrolysis of NaCl solution wirh inen electrodes for cefiain period of lT"*:]:-'-?1,:T"i:::*)::1ll:X:e*cLrot) uu 'r' /ur rrr. 'rrii"n'r'intt'eetectrolliic(ell?(At'\^t'ofcu=63'6)(A) 40 (B) 50 (c) 60 (D) 2sUsing electrolltic method, ilcost ofprcduction of lL ofoxyge arSTPisRs x'thecoslofproductioilof10L of

>5CPP - CHEI\IICAL KINBTICS. NUCLtrAR CIIEMISTRY' ELECTROCIIENIISTRY 50 cG?'re-

(B) away from the anode(D) iowards anode and cathodeA 1.0 M with respect to each of metal halides AXr, BX:' CXr and DX: lt-"]:tl':''*O ""itl]T:l:I",:l::i?IF E". = r.50 v, E:,-.-:0.34, E: = 0.74V, E: = 2.37 V, the correct sequence in which thevarious meials are deposited at the cathode rs(A) A. B. t. D (B) D, C. B, A (c) A, B, c (D) C, B. ACiven thet 2CI =CL +2e. E"=-l 36V; Hro-' + 2ll* + 2e r' Eo= 123 V on electrolysing I MNaCI solutionir,r,',*I "i*""a"., ,rt,;"r, orrl" rotto*lirji, co*ecr regardirg liberation of electrol)4ic products?i^;;il;;,;r;r, lel cattoae: ni. o, (c)Anode:o' (D)Anode:cl'lnelectroiyticreductionolanitroarenc$ith50oZcurrentelficiency,20,50goflhecompoundisreducedby2xqiioo i oi .'..,,i. . L.rge. I he rrrohr md'' oltl e co lpuJird i':i^;;i,;o- (B) r0.2ss (c) 121'00s (D)6i 509^1.,,1.1^r,oeh,ner\conlainin9.5.0lolH:So,solutioniJoTeml(Jlblqb5\lU.s.tra'teld5cunento[100il.,tt;;,"; ;i;;" "i,r" '"i''i"" *,."i"'''s con'ranr' lormdlin^or H'soi

\\ illi[ ri.""." ti ,",ii - - ietln",""" t'v o 2o (C) decrease bv 0'40 (D) remain unchangedAcidulated water is electrolysed by i A current for 16 minutes aDd 5 seconds using inert electrodes- The volume

hydrogen at STP will be:(A) 10x (B) Jl6 (c) I0132 (D) 10x/2The charge requiled for the oxidation of one mole of Mnroa to NInOI io alkalirle mediuln is (assume l00c%

ln an electrolytic cell, electmns move(A) towards anode(C) away from the cathode

current efficiency):(A) l0/3 - (B) 6F (c) l0 F (D) 4F-+8250 C ol ecc'riciD ua: requir.d lo depo'll 'r I lrtr Loop


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I5. Thc \'aiue ofthe reaclion quotient, Q,(A) 12.s(c) 0.20Which ofthe foilowing is always true(A) EL|| > 0,4G" < 0 and Q> K.(C) ELr > o,AC'> o and Q> K.

Consider the gaivanic cellPbG) lPb:;(xjN1) ll Cu:; (x,M) | cu(t

tbr lhe cell C(s) Cr:;(0 ri\'1)(B) 0.08(D) 5.0

E Lr, : o'ri v

cu:;10.i N,)icur\)

16. regading the spontaneity of reactioo occurring in a galvanic cell?(B)E:er > 0,AGo A(s)Bt+e J B(s)Xr(g) r2e + 2XWhich of ihe lollo\\ing statements is not true?(A) xlg) *i]l oxidize both A and B

(B) 0.592 V(D) 0.592 VE"=010vEa = - 2j7YE"= 1.08 V(B) A:- will oxidize B

(C) The reaction 2X ( I.0M) + Ar- (1.0 M) --- + X: ( I a1m) + A(s) will be spontaneous(D) The oxidizing po\\'er ofAr.. Bt and X:(g) is in the order : B'< Ar- < X,

The EMF ofthe cell Pt, Clr(g) (pr atm) | Cl( Ilvl)/C11 (praim). Pt rvil be positive when:(A) p, > p, (B) pr - p,(C) p' < p, (D) none oftheseWhat is the EMF of the gahanic cell (K,p of A gCl = 1.0 r I 0 r'r)Ag, Agcl(s) | I N4 KCI(aq) i iM AsNOdaq) I Ag

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.80 g of metal M is depositd at the catbode b) passing 0.2 F ofchloride. The fomlula olthe metal chloridc: (Atomic .rass ofM : 57)(c) MCI:relectriclty through the solutioD of melal(D) MCrlA) MCI (B) MCrz

The halfcell poteniial for the quinhydrone electrode

ln acidic medium, MnOz is an oxidant aslMnor(s) + 4H. +2e -> Mn2* + 2HrOllrhe fH ofrhe solution is decrea.ed b) one urit. .he eleirrode poterrt alhalfcellPt. MnO.. Nln']- $ rll change bi(A),0.1r 8 v (B) 0.r r8 v (c) 0.2r6 v

olthe(D) 0.236 V

setupatpH=4will be (quinhydrone = I : 1 ,nolecular compo ndolquinone(Q)andhydroquinone(QH2)'E :0.6q9 v)(A) 0.699 v (B) 0.463 V(c) 0.93s v (D) 0.817 V

O U}IA)[r rl . '." "-[CYY OJIGiven thai E i,2.,", : 0.3'1 V: E""*/Aq : o.so V; E;s,./i/a:-237vandE:3./A - r '66 v, in which of thelollo$ inc. ccll" lhe 'landard ire. ene'g) Jr crea\c ir md \irnum:(A) Ms i-Mg']- (1M) lcu'?.(1M) cu (B)MglMs'?'(lM)lAg (lNa)lAgicjeilaettr'rvri,qr'.(ru)let (D)culcur-(1M)lAg(1M)lAsCiven the cell reactions\IX(s)-e - r \'I(s.) - X(.,r);and MLq)+ e- -----+ M(s);the so,ubilitv oi l\'lx solid at 298 K is(A) t.o x t0lro m.l L r(C) L0 \ I0 rnol L I

E" = 0.207 VE = 0.799 V(B) l.0x l0'mol L1D1 1.0 r l0'mol Ll

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Which ofthe follo\\,ing statemeflts is not corect during the \Yorking ol he cell:cuG) | Cu al) (M,) I cr a;) (M,l I cu(s)M1 < M1, M's being the molarities of Cu i";)(A) E..l decreases and falls ultimately to zeroigi M, in".""... una Na, decreases dueto direc transfer oICu:' ionsiCiU, ;n"r.u.". au",o oxidation ofCu(s) and N{r dec -eases due to reaction olCur- ions(D) ELr = 0.0 vH, analD: gases at a pressure o1'l atnt each at 25"C are in equilibriurr wilh a sclution containing H* and D- ions.lfE 3*/D, = -0.003 v, calculaie 1og [D-]/[Ht](A) 5.0 (B) o.so(c) o.os (D) 0.005

31. Givenrhat:E'aq,/Ao=0.80vand[Ag.]=l0rM;E;sr./Eq=0.785vandiHs;'1=10 M rvhich istrueof forthe cell reactior 2llg(l) + 2Ag-(aq) + 2A8(, + Hg r+ (aq)(A) the forward reactiorr is sPontaneous (B) the back\\ard ]action is sportlaneous(C) E ccll= 0.163 (D)Ecell=1.58s


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The equilibrium constant for the disproportioationV; Ei,r*,", = 0.16 V) is:(A) 1,2 x l0{(C) 6 x 106

ion: 2cuaq)+ Cu(s) + Cua-q) at 25"C104x 106(B)6x(D) 1.2

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The electrical work done during the reaction1 36 v;Eir",,nn.", - 0 27 v; Pcr2 = l atm'(A) 210.37 kl mol I(C) 420.74 kJ mol 'Consider the cell: X(s)lXL-q) lY;q) Y(s)IfEi3-/x = 1.66 V and E02+/y:0.34 V,in the above cell at 25"C, is:(A) 67.56G) 242.70

CHEMICAL KINETICST-+co is equal to(A) Energy ofactivation ofthe rcaction

at 298Ki 2Hs(l) + Cl,(g) r H&Clr(s), ' ct2 tcti05.185 klmol I110.37 kJ mol I

logarilhm tro lhe base l0l olequilibr um con"rrnl ofthe 1et reacrion10r.35168.92

(B) Fraction ofmolecu|es in the activared ffi

(B)(D)

(B)(D)

I The ratio oi the raie constant of a reaction at any tempeEiture T to dre rate constant(C) Average life ofthe reaction(D) Pre-exponentis factor in tle Arrhenius equation

2. The mte constant ofa reaction: A--'>B+Cat27"C is3.0x l0 js-r at 27"C and ar rbis ternperaarc 15x l0rpercent of the reactant molecules are able to cross-oler the P.E. barrier. The maiimum rate mDshnt of thereaction is(A) 4.5 x 10-'gs-' (B) 4.5 x l0 rr s'l (C) 0.2 s I (D)20s'J, hor a lrrsl orJer reaclron: A : B. shose concertration rs.time curve is as shown in the figure. The rate constant is equal :to:(A) 41.58 h-' @)4.158 s ' E{C) Ll55 . t0'.r 1D)0.9.} min' 3

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For the gaseous reaction A,n, -+48,n, + 3C(q) is found to be first order with respect to A. lf at the starting thetotal pressure was 100 mm Hg and after 20 minutes it is found to be 400 mm Hg. The rate constant ofthe rcactionis:(A) 20 min l (B) i.2 x 103 sec 1 (C) 5.7x 10 a sec 1 (D) 40 min 'The decomposition ofozone is believed to occur by the mechanisrn:O" EBHr O, + O (fasi)O + 03 J O, (slow)When tie concentration of 02 is increased, then the rate

(C) remains sarre (D) c6nlot be predrcted

In the sequeDce of the reactid 4 xt ,g xz ,6 K: .D, girrn tnar K1


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,y'hat rvill be the iraction ofmolecule having energ}- equalto or greaierthan aciivation energy E,?(B) A (c) Ae t, Pr (D) e o'

(C) secondHalflife ofa chemical reaction at a particular concentration is 50 min. When the concentration oflhe .eactant isdoubled, the halflife becomes 100 min, then the order ofthe reaction is:(A) K

lcH3crI0.20.40.4

toH'l0.10.1o2

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(A) zero (B) fiIst (D) thirdDecomposition of ,A f'ollows firsi order kinetics by tlre following equaliorl4A,n, +B,n, + 2C,n,ilat initial, the total pressure is 800 mm of Hg and after l0 minutes it is loundhalflife ofA?(A) 5 minutes (B) 10 mioutes (C) 7.5 minutes (D) 20For the reactionCH3Ct{.q)+oHi"q)E ErE. CH-oH1"o1 + C11"qrThe kjnetic data are as given below:

to be 650 mm ofHg. What is theminuLes

+d[CH3OH]/dt (M mini)2x10 \4 x '10-38x10 3

E. and dFI values ofreactions Rl, R, R3 and Racarried oul at the same ternperal'lre are as given below:R. E,=40k.l rnoI \H=-EokJmolR2 E. = 20 kJ mol-1, ,\H = 30 kJ mol-rR3 E. = 60 kJ mol 1, ,\H = +40 kJ mollR4 E" = 30 kJ mol-], ^H = +20 kJ mol-lAt e given tenperature and assuming that the backward reactions clall these reactions have the same liequencyfactor, the rates of R1, R2, R3 and R.a in their respective back*'ard reacl;ons are in the increasing order of(A) R,

chem kinetics worksheet

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