Question 2 : The correct order of the stoichiometries of $AgCl$ formed when $AgNO_{3}$ in excess is treated with the complexes: $CoCl_{3}.6NH_{3}, CoCl_{3}.5NH_{3}, CoCl_{3}.4NH_{3}$ respectively is:

Question 3 : Which of the following is the cell reaction that occurs when the following half-cells are combined?<br>$I_2+2e^-\rightarrow 2I^-(1M)$; $E^o=+0.54$V<br>$Br_2+2e^-\rightarrow 2Br^-(1M); E^o=+1.09$V<br>

Question 4 : Saturated solution $K{ NO }_{ 3 }$ is used to make salt bridge because:

Question 5 : Given that the standard reduction potentials for ${ { M }^{ + } }/{ M }$ and ${ { N }^{ + } }/{ N }$ electrodes at $298 K$ are $0.52 V$ and $0.25 V$ respectively. Which of the following is correct in respect of the following electrochemical cell?<br>$M | { M }^{ + } || { N }^{ + } | N$

Question 6 : <p> The standard electrode potentials ${\text{E}}_{{{\text{I}}_2}/{1^ - }}^ \circ ,{\text{E}}_{{\text{B}}{{\text{r}}^ - }/{\text{B}}{{\text{r}}_2}}^ \circ $ and ${\text{E}}_{{\text{Fe/F}}{{\text{e}}^{2 + }}}^ \circ $ are respectively $ + 0.54{\text{V,}} - 1.09{\text{V}}$ and 0.44 V. On the basis of the above data which of the following process is nonspontaneous?</p>

Question 7 : A reaction:<div><br/>$\displaystyle \dfrac{1}{2}H_2(g)\, +\, AgCl(s)\, \rightleftharpoons\, H^{\oplus}(aq)\, +\, Cl^{\ominus} (aq)\, +\, Ag(s)$ occurs in a galvanic cell. </div><br/><div>The structure of the cell will be:</div>

Question 8 : The reaction,<br/><div> $(1/2) H_2 (g) + AgCl(s) = H^+ (aq) + Cl^- (aq) + Ag (s)$ occurs in the galvanic cell </div><br/><div> The correct cell representation is given by _____________.</div>

Question 9 : Assertion: The conductivity of electrolytic solutions increases with increase of temperature. Reason: Electronic conductance decreases with increase of temperature.

Question 10 : Saturated solution of $KNO_3$ is used to make ' salt-bridge' because:

Question 11 : A solution containing one mole per litre of each $Cu(NO_3)_2$, $AgNO_3, Hg_2(NO_3)_2$ and $Mg(NO_3)_2$ is being electrolysed by using inert electrodes. The values of standard electrode potentials in volts(reduction potential) are.<br>$Ag^+/Ag=+0.80, Hg^{2+}_2/2Hg =+0.79$<br>$Cu^{2+}/Cu=+0.34, Mg^{2+}/Mg =-2.37$<br>With increasing voltage, the sequence of deposition of metals on the cathode will be:<br>

Question 14 : In which of the following cells, use of salt bridge to eliminate liquid junction potential is not necessary?

Question 15 : Consider the following half-cell reactions and associated standard half-cell potentials and determine the maximum voltage that can be obtained by combination resulting in spontaneous processes:<br>$AuBr_{4}^{-}(aq) + 3e^{-} \rightarrow Au(s) + 4Br^{-}(aq); E^{\circ} = -0.86\ V$<br>$Eu^{3+}(aq) + e^{-} \rightarrow Eu^{2+}(aq); E^{\circ} = -0.43\ V$<br>$Sn^{2+}(aq) + 2e^{-} \rightarrow Sn(s); E^{\circ} = -0.14\ V$<br>$IO^{-}(aq) + H_{2}O(l) + 2e^{-}\rightarrow I^{-}(aq) + 2OH^{-}(aq); E^{\circ} = + 0.49\ V$

Question 16 : The equivalent conductance of $\cfrac{M}{32}$ solution of a weak monobasic acid is $8.0 \ mhos \ cm^2$ and at infinite dilution is $400 \ mhos \ cm^2$. The dissociation constant of this acid is:<br/>

Question 17 : Assertion: In electrochemical cell, we can not use KCl in the salt bridge if anodic or cathodic compartment consists of Ag$^+$ or Pb$^{2+}$ ion. Reason: Salt bridge is employed to maintain the electrical neutrality and to minimize the liquid-liquid junction potential.

Question 19 : Given below are the half-cell reactions:<br/>$Mn^{2+} + 2e^- \to Mn; E^o = -1.18V$<br/>$2(Mn^{3+} + e^- \to Mn^{2+}); E^o = +1.51V$<br/>The $E^o$ for $3Mn^{2+} \to Mn +2Mn^{3+}$ will be:

Question 20 : A steady current of $10.0$ Amps is passed through a nickel production cell of $15$ minutes.<br>Which of the following is the correct expression for calculating the number of grams of nickel produced?<br>Note:<br>$\bullet 1\ faraday = 96,500\ Coulombs$<br>$\bullet$ The electroytic cell involves the following half-reaction:<br>$Ni_{(aq)}^{2+} + 2e^{-} \rightarrow Ni_{(s)}$<br>

Question 21 : In a voltaic cell, if iron and silver electrodes are connected with each other then current flows:<br/>

Question 22 : What will be $\Delta H$ for the reaction; $Ag(s)+\dfrac{1}{2}Hg_2Cl_2(s)\rightarrow AgCl(s)+Hg(l)$ at $25^0c$, if this reaction can be conducted in a cell for which the emf = 0.0455 volt at this temperature with temperature coefficient $3.389\times10^{-4} volt\, deg^{-1}$?

Question 23 : Consider a galvanic cell using solid $Cu$ and $Fe$ metals with their corresponding solutions.<br>What is the $E^{\circ}_{cell}$?<table class="wysiwyg-table"><tbody><tr><td>Standard Potential (V)</td><td>Reduction Half-Reaction</td></tr><tr><td>$2.87$</td><td>$F_{2}(g) + 2e^{-} \rightarrow 2F^{-}(aq)$</td></tr><tr><td>$1.51$</td><td>$MnO_{4}^{-}(aq) + 8H^{+}(aq) + 5e^{-}\rightarrow Mn^{2+}(aq) + 4H_{2}O(l)$</td></tr><tr><td>$1.36$</td><td>$Cl_{2}(aq) + 3e^{-} \rightarrow 2Cl^{-}(aq)$</td></tr><tr><td>$1.33$</td><td>$Cr_{2}O_{7}^{2-} (aq) + 14H^{+}(aq) + 6e^{-} \rightarrow 2Cr^{3+}(aq) + 7H_{2}O(l)$</td></tr><tr><td>$1.23$</td><td>$O_{2}(g) + 4H^{+}(aq) + 4e^{-}\rightarrow 2H_{2}O(l)$</td></tr><tr><td>$1.06$</td><td>$Br_{2}(l) + 2e^{-} \rightarrow 2Br^{-}(aq)$</td></tr><tr><td>$0.96$</td><td>$NO_{3}^{-}(aq) + 4H^{+}(aq) + 3e^{-}\rightarrow NO(g) + H_{2}O(l)$</td></tr><tr><td>$0.80$</td><td>$Ag^{+}(aq) + e^{-} \rightarrow Ag(s)$</td></tr><tr><td>$0.77$</td><td>$Fe^{3+} (aq) + e^{-} \rightarrow Fe^{2+}(aq)$</td></tr><tr><td>$0.68$</td><td>$O_{2}(g) + 2H^{+}(aq) + 2e^{-}\rightarrow H_{2}O_{2}(aq)$</td></tr><tr><td>$0.59$</td><td>$MnO_{4}^{-}(aq) + 2H_{2}O(l) + 3e^{-}\rightarrow MnO_{2}(s) + 4OH^{-}(aq)$</td></tr><tr><td>$0.54$</td><td>$I_{2}(s) + 2e^{-}\rightarrow 2I^{-}(aq)$</td></tr><tr><td>$0.40$</td><td>$O_{2}(g) + 2H_{2}O(l) + 4e^{-} \rightarrow 4OH^{-}(aq)$<br></td></tr><tr><td>$0.34$</td><td>$Cu^{2+}(aq) + 2e^{-} \rightarrow Cu(s)$</td></tr><tr><td>$0$</td><td>$2H^{+}(aq) + 2e^{-}\rightarrow H_{2}(g)$</td></tr><tr><td>$-0.28$</td><td>$Ni^{2+}(aq) + 2e^{-}\rightarrow Ni(s)$</td></tr><tr><td>$-0.44$</td><td>$Fe^{2+}(aq) + 2e^{-}\rightarrow Fe(s)$</td></tr><tr><td>$-0.76$</td><td>$Zn^{2+}(aq) + 2e^{-}\rightarrow Zn(s)$</td></tr><tr><td>$-0.83$</td><td>$2H_{2}O(l) + 2e^{-}\rightarrow H_{2}(g) + 2OH^{-}(aq)$</td></tr><tr><td>$1.66$</td><td>$Al^{3+}(aq) + 3e^{-}\rightarrow Al(s)$</td></tr><tr><td>$-2.71$</td><td>$Na^{+}(aq) + e^{-} \rightarrow Na(s)$</td></tr><tr><td>$-3.05$</td><td>$Li^{+}(aq) + e^{-}\rightarrow Li(s)$</td></tr></tbody></table>

Question 25 : The reaction taking place in the cell $Pt|\underset {1\ atm}{H_{2}(g)}|HCl(1.0\ M)|AgCl|Ag$ is:

Question 26 : Amongst the following, the form of water with the lowest ionic conductance at $298 K$ is :

Question 28 : In dry cell the reaction which takes place at the zinc anode is:

Question 29 : A galvanic cell is constructed using two Hydrogen electrodes. Emf is highest when the pH of the solutions at anode and cathode is _____ and ______ respectively.

Question 30 : In an electrochemical cell, reduction takes place at anode BECAUSE oxidation always takes place at the cathode.

Question 31 : The rate law of the reaction $A+2B\rightarrow Product$ is given by $\dfrac{d\left[dB\right]}{dt}=k\left[B\right]^{2}$ If A is taken in excess, the order of the reaction will be:

Question 32 : The rate equation for the reaction $2\mathrm{A}+\mathrm{B}\rightarrow \mathrm{C}$ is found to be: <div>Rate $=\mathrm{k}[\mathrm{A}][\mathrm{B}]$.<br/></div>

Question 33 : In which of the following cases, does the reaction farthest to completion?

Question 34 : If activation energy, E_a of the reaction is equal to RT then<br>

Question 35 : In which of the following reactions of the following orders the molecularity and order can never be same?

Question 36 : ${H}_{2}+{Br}_{2}\rightarrow 2HBr$. <div> The rate law is $\cfrac{dx}{dt}=k[{H}_{2}]^{1/2}{[{Br}_{2}]}^{1/2}$:<br/></div><div> On increasing the concentration of ${Br}_{2}$ four times, by how much times the rate of reaction will change? <br/></div>

Question 37 : Select the intermediate in the following reaction :<br>2O₃&#8213;&rarr; 3O₂<br>Step (i) O₃(g) <img style='object-fit:contain' src='https://storage.googleapis.com/teachmint/question_assets/JEE%20Main/5e799d9fced10523befee588' height='16' width='47' > O₂(g) + O(g)<br>Step (ii) O(g) + O₃(g) &#8213;&rarr; 2O₂<sub><br>

Question 38 : A hypothertical reaction, A₂ + B₂{tex}\rightarrow{/tex}2AB follows the mechanism as given below ;<br>A₂<img style='object-fit:contain' src='https://storage.googleapis.com/teachmint/question_assets/JEE%20Main/5e799d8be89a3d21421700f2' height='11' width='26' >A + A ...(Fast)<br>A + B₂{tex}\rightarrow{/tex}AB + B ...(Slow)<br>A + B {tex}\rightarrow{/tex}AB ... (Fast)<br>The order of the overall reaction is -<br>

Question 39 : For a reaction pA + qB $\rightarrow$ Products, the rate law expression is r = k[A]$[B]^m$, Then:

Question 41 : The following are the data for the reaction <div> <br/></div><div> $A+B\rightarrow $ products </div><div> <br/></div><div> [A] [B] Initial rate $(mol\, L^{-1}s^{-1})$<br/> (i) 0.1 M 0.1 M $4.0\times 10^{-4}$<br/> (ii) 0.2 M 0.2 M $1.6\times 10^{-3}$<br/> (iii) 0.5 M 0.1 M $1.0\times 10^{-2}$<br/> (iv) 0.5 M 0.5 M $1.0\times 10^{-2}$ <div><br/><div>The rate constant of the reaction is _________ .<br/><br/></div></div></div>

Question 42 : In the first order reaction {tex} \mathrm { t } _ { 99.9\%} {/tex} is 60 minute. {tex} \mathrm { t } _ { 50 \% } {/tex} of the reaction would be nearly

Question 43 : For reaction RX + OH^-&rarr; ROH + X^-, Rate expression is R = 4.7 &times; 10^-5 [RX][OH^-] + 2.4 &times; 10^-5 [RX].What % of reactant react by <img style='object-fit:contain' src='https://storage.googleapis.com/teachmint/question_assets/JEE%20Main/5e799dade89a3d214217013e' height='23' width='25' >mechanism when [OH^-] = 0.001 molar -<br>

Question 44 : A drop of solution (volume 0.05 mL) contains 3.0 &times; 10^-6 moles of H⁺. If the rate constant of disappearance of H⁺ is 1.0 &times; 107 mole litre^-1 sec^-1. How long would it take for H⁺ in drop to disappear :<br>

Question 45 : <table class="table table-bordered"><tbody><tr><td> Volume of $N_2$ (in cc)</td><td> Time (in minutes)</td></tr><tr><td> 6.25</td><td> 10</td></tr><tr><td> 9</td><td> 15</td></tr><tr><td> 11.4</td><td> 20</td></tr><tr><td> 13.65</td><td> 25</td></tr><tr><td> 35.05</td><td> $\infty$</td></tr></tbody></table><div>The following data is for the decomposition of ammonium nitrite in aqueous solution. </div><div> The order of the reaction is:<br/></div>

Question 46 : What is the order of a chemical reaction $A+2B\xrightarrow {k} C$, if the rate of formation of $C$ increases by a factor of 2.82 on doubling the concentration of $A$ and increases by a factor of 9 on tripling the concentration of $B$?

Question 47 : The rate of a certain reaction is given by, rate $=k{ \left[ { H }^{ + } \right] }^{ n }$. The rate increases 100 times when the pH changes from 3 to 1. The order $\left( n \right) $ of the reaction is:

Question 48 : <div> The following are the data for the reaction <br/></div><br/><div> $A+B\rightarrow $ products </div><br/><div> [A] [B] Initial rate $(mol\, L^{-1}s^{-1})$</div><div>(i) 0.1 M 0.1 M $4.0\times 10^{-4}$</div><div>(ii) 0.2 M 0.2 M $1.6\times 10^{-3}$</div><div>(iii) 0.5 M 0.1 M $1.0\times 10^{-2}$</div>(iv) 0.5 M 0.5 M $1.0\times 10^{-2}$ <br/><div>The reaction rate when the concentration of A and B are 0.4 M and 0.7 M respectively :<br/></div>

Question 49 : Which one of the following statements for the order of a reaction is incorrect?<br/>

Question 50 : The reaction $A(s) \rightarrow 2B(g) + C(g) $ is first order. The pressure after $20$ min. and after a very long time are $150$ mm $Hg$ and $225$ mm $Hg$. The value of rate constant and pressure after $40$ min. are?

Question 51 : What will be the order of the reaction given below?<br/><br/><div>$NH_4CNO\rightarrow NH_2CONH_2$<br/><br/><div>The reaction is completed in three steps as:<br/><br/></div><div>(i) $NH_4CNO\rightleftharpoons NH_4NCO$ (fast equilibrium)<br/><br/></div><div>(ii) $NH_4NCO\rightleftharpoons NH_3+H-N=C=O$ (fast equilibrium)<br/><br/></div><div>(iii) $NH_3+H-N=C=O\rightarrow NH_2CONH_2$ (slow equilibrium)<br/></div></div>

Question 52 : For the chemical reaction A + 2B $\rightarrow$ C, rate of the reaction is increased by 2.82 times when the concentration of A is doubled and increased by 9 times when the concentration of B was tripled. What is the order with respect to B, A, and the total order ?

Question 53 : A catalyst lowers the activation energy for a certain reaction from $83.314$ to $75 \,kJ \,mol^{-1}$ at $500\,K.$ What will be the rate of reaction as compare to uncatalysed reaction ? Assume other things being equal.

Question 55 : At a certain temperature,the half life periods for the catalytic decomposition of ammonia were found to be as; <br/>Pressure (mm) 50 100 200<br/>$t_{ 1/2}$ 3.52 1.92 1.0 <br/>What is the order of reaction?

Question 56 : An aqueous solution $0.10M\,H_2S$ ans $0.20M\, HCl$. If the equilibrium constants for the formation of $HS^-$ from $H_2S$ is $1.0\times 10^{-7}$ and that of $S^{2-}$ from $HS^-$ ions is $1.2\times 10^{-13}$ then the concentration of $S^{2-}$ions in aqueous solution is:

Question 57 : The order of a reaction with rate equals $kC_{A}^{3/2} C_{B}^{-1/2}$ is:

Question 58 : What will be order of reaction and rate constant for a chemical change having t_50% v/s log conc. curve as -<br><img style='object-fit:contain' src='https://storage.googleapis.com/teachmint/question_assets/JEE%20Main/5e799db9a2bddf222e0af764' height='106' width='128' >

Question 60 : Statement-1 : The ratio of for third order reaction is equal to 5 : 1 <br>Statement-2 : t_1/2 & t_3/4 of a reaction depends only on order, not on the concentration of reactant.<br>

Question 61 : For the reaction $A+B\rightarrow products$, doubling the concentration of $A$ the rate of the reaction is doubled, but on doubling the concentration of $B$ rate remains unaltered. The over all order of the reaction is:

Question 62 : The rate constant of reaction $2A+B\rightarrow C$ is $2.57\times {10}^{-5}$ $litre$ ${mole}^{-1}$ ${sec}^{-1}$ after $10$ sec. $2.65\times {10}^{-5}$ $litre$ ${mole}^{-1}$ ${sec}^{-1}$ after $20$ sec and $2.55\times {10}^{-5} litre.$ ${mole}^{-1}$ ${sec}^{-1}$ after $30$ sec. The order of the reaction is:

Question 63 : The reaction $A(g) + 2B(g) \rightarrow C(g) + D(g)$ is an elementary process. In an experiment, the initial partial pressure of A and B are $P_A = 0.60$ and $P_B = 0.80$ atm. When $P_C = 0.2$ atm, the rate of reaction relative to the initial rate is:

Question 64 : Consider the reaction:<br>$Cl_2(aq) +H_2S(aq) \to S(s) + 2H^+(aq) + 2Cl^-(aq)$<br>The rate equation for this reaction is rate $=k\, [Cl_2] [H_2S]$<br>Which of these mechanisms is /are consistant with this rate equation?<br>(A) $Cl_2 + H_2S \to H^+ + Cl^-+Cl^+ + HS^-$ (slow)<br> $Cl^+ + HS^- \to H^+ + Cl^- + S$ (fast)<br>(B) $H_2S \rightleftharpoons H^+ + HS^-$ (fast equilibrium)<br> $Cl_2+HS^-\to 2Cl^-+H^+ + S$ (slow)<br>

Question 66 : When a graph between log K and 1/T is drawn a straight line is obtained. The point at which line cuts y -axis and x -axis respectively correspond to the temp :<br>

Question 67 : For a given reaction. $t_{1/2}=\dfrac{1}{Ka}$. The order of the reaction is:

Question 68 : The rate of a chemical reaction doubles for every <b>10&deg;C</b> rise of temperature. If the temperature is raised by <b>50&deg;C</b>, the rate of the reaction increases by about :<br>

Question 69 : For a reaction $\dfrac{dX}{dt}=K[H^{+}]^{n}$. If $pH$ of reaction medium changes from two to one, the rate becomes 100 times of the value at $pH$ $=$ 2. The order of reaction is:<br/>

Question 70 : For a certain reaction the rate law is rate $= k [C]^{3/2}$. If the rate of the reaction is $0.020$ mol L$^{-1}$s$^{-1}$ when $[C]$ = $1.0$ M, what is the rate when $[C]$ = $0.60$ M?

Question 71 : For the reaction $NO_{2}+CO\rightarrow CO_{2}+NO$ the experimental rate expression is $-\frac{dc}{dt}=k[NO_2]^2$ the number of molecules of CO involves in the slowest step will be:<br/>

Question 72 : For reaction $A \rightarrow B,$ the rate constant $k_1 = A_1 (e^{-E_{a_1} / RT})$ and for the reaction $X \rightarrow Y,$ the rate constant $k_2 = A_2 (e^{-E_{a_2}} / RT).$ If $A_1 = 10^9. A_2 = 10^{10}$ and $E_{a_1} = 1200 \,cal / mol,$ then the temperature at which $k_1 = k_2$ is: $(Given; R = 2\,cal / K-mol)$

Question 74 : Assertion: Complex reaction takes place in different steps and the slowest step determines the rate of reaction. Reason: Order and molecularity of a reaction are always equal.

Question 75 : A schematic plot of in K_eq versus inverse of temperature for a reaction is shown below<br><img style='object-fit:contain' src='https://storage.googleapis.com/teachmint/question_assets/JEE%20Main/5e799e07e89a3d214217020d' height='159' width='225' ><br>The reaction must be<br>

Question 78 : The reaction: <img style='object-fit:contain' src='https://storage.googleapis.com/teachmint/question_assets/JEE%20Main/5e799d3ea2bddf222e0af540' height='24' width='195' > has been assigned to follow following mechanism.<br><img style='object-fit:contain' src='https://storage.googleapis.com/teachmint/question_assets/JEE%20Main/5e799d3ea2bddf222e0af541' height='75' width='241' ><br>The rate constant of step II is 1.2 x 10^-4mol^-1L.min^-1 while equilbrium constant of step I is 1.4 x 10^-2 .What is the rate of reaction when concentration of NO and H₂ each is 0.5 mole L^-1<br>

Question 79 : The reaction A + 2B + C $\rightarrow$ 2D + E is found to be 1, 2 and Zero order with respect to A,B and C respectively. What will be the final rate, if concentration of each reactant is doubled?

Question 80 : For the reaction, $2{ N }_{ 2 }{ O }_{ 5 }\longrightarrow 4N{ O }_{ 2 }+{ O }_{ 2 }$ the value of rate constant and rate of reaction are respectively $3\times { 10 }^{ -5 }{ s }^{ -1 }$ and $2.4\times { 10 }^{ -5 }\ M{ s }^{ -1 }$. The concentration of ${ N }_{ 2 }{ O }_{ 5 }$ (in mol L $^{ -1 }$) will be: