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question_answer1) The standard free energy change for the reaction: \[{{H}_{2(g)}}+2AgC{{l}_{(s)}}\to 2A{{g}_{(s)}}+2H_{(aq)}^{+}+2Cl_{(aq)}^{-}\] is \[-10.26kcal\,mo{{l}^{-1}}\] at \[25{}^\circ C\] . A cell using above reaction is operated at \[25{}^\circ C\] under \[{{P}_{{{H}_{2}}}}=1atm\], \[[{{H}^{+}}]\] and \[[C{{l}^{-}}]=0.1\]. Calculate e.m.f. of cell.
question_answer2) The e.m.f. of cell \[Zn\left| ZnS{{O}_{4}} \right|\,\,\left| CuS{{O}_{4}} \right|Cu\] at \[25{}^\circ C\] is 0.03V and the temperature coefficient of e.m.f. is \[-1.4\times {{10}^{-4}}V\] per degree. Calculate heat of reaction for the change taking place inside the cell.
question_answer3) EMF diagram for iron is given as: \[\underset{\left( Fe=+6 \right)}{\mathop{E{}^\circ \left( volts \right)Fe{{O}_{4}}^{2-}}}\,\xrightarrow{+2.20}\underset{\left( Fe=+3 \right)}{\mathop{F{{e}^{3+}}}}\,\] \[\xrightarrow{+0.77}\underset{\left( Fe=+2 \right)}{\mathop{F{{e}^{2+}}}}\,\xrightarrow{-0.445}\underset{\left( Fe=+0 \right)}{\mathop{F{{e}^{0}}}}\,\] Determine the value of \[E_{FeO_{4}^{2-}/F{{e}^{2+}}}^{0}\].
question_answer4) Calculate the maximum work that can be obtained from the cell. \[Zn\left| Z{{n}^{2+}}\left( 1M \right) \right|\,\,\,\left| A{{g}^{+}}\left( 1M \right) \right|Ag\] Given that \[E_{Zn/Z{{n}^{2+}}}^{0}=0.76V\] and \[E_{Ag/A{{g}^{+}}}^{0}=-\,0.80V\]
question_answer5) For the cell process: \[Sn\left( s \right)+P{{b}^{+2}}\left( aq \right)\to \]\[Pb\left( s \right)+S{{n}^{+2}}\left( aq \right)\] Calculate ratio if \[P{{b}^{+2}}\] to \[S{{n}^{+2}}ion\] concentration for spontainity. Given \[E_{S{{n}^{2+}}/Sn}^{0}=-0.136V\] \[E_{P{{b}^{2+}}/Pb}^{0}=-0.126V\]
question_answer6) A galvanic cell is consisted of metallic zinc plate immersed in \[0.1\,M\,Zn{{\left( N{{O}_{3}} \right)}_{2}}\] solution and a lead plate immersed in 0.02M \[Pb{{\left( N{{O}_{3}} \right)}_{2}}\] solution. Calculate emf of the cell. Given : \[E_{Z{{n}^{2+}}/Zn}^{0}=-0.76V\] and \[E_{P{{b}^{2+}}/Pb}^{0}=-0.13V\]
question_answer7) Calculate the potential of the standard Iron-Cadmium cell after the reaction has proceeded to 80% completion. Initially 1 M of each taken and \[E{}^\circ \] for cell = 0.04 V. \[Fe\left( s \right)\left| F{{e}^{+2}} \right|\,\,\,\left| C{{d}^{+2}} \right|Cd\]
question_answer8) The e.m.f. of the cell, \[{{H}_{2}}\left( g \right)\left| Buffer \right|\,\,\left. {} \right|\] Normal calomel electrode is 0.6885 volt at \[25{}^\circ C\] when barometric pressure is 760 mm Hg. What is pH of the buffer solution. \[E{{{}^\circ }_{calomel}}=0.28volt\]
question_answer9) A 200 W, 110V incandescent lamp is connected in series with an electrolytic cell of negligible resistance containing a solution of \[ZnC{{l}_{2}}\] . What weight of Zn will be deposited from the solution on passing current for 30 minutes? (At.wt. of Zn = 65.4)
question_answer10) All the energy released from the reaction \[X\to Y,\]\[{{\Delta }_{r}}G{}^\circ =-193kJ\,mo{{l}^{-}}\] is used for oxidizing \[{{M}^{+}}\] as\[{{M}^{+}}\to {{M}^{3+}}+2{{e}^{-}},\]\[E{}^\circ =-0.25V\]. Under standard conditions, the number of moles of \[{{M}^{+}}\] oxidized when one mole of X is converted to Y is \[[F=96500C\,mo{{l}^{-1}}]\]
question_answer11) The molar conductivity of a solution of a weak acid\[HX\text{ }\left( 0.01\text{ }M \right)\] is 10 times smaller than the molar conductivity of a solution of a weak acid\[HY\text{ }\left( 0.10\text{ }M \right)\]. If \[\lambda _{{{X}^{-}}}^{0}\approx \lambda _{{{Y}^{-}}}^{0}\], the difference in their \[p{{K}_{a}}\] values, \[p{{K}_{a}}\left( HX \right)-p{{K}_{a}}\left( HY \right)\], is (consider-degree of ionization of both acids to be <<1)
question_answer12) For the following electrochemical cell at 298 K, \[Pt\left( s \right)\left| {{H}_{2}}\left( g,1bar \right) \right|\] \[\left. {{H}^{+}}\left( aq,1M \right) \right|\] \[\left| {{M}^{4+}}\left( aq \right),{{M}^{2+}}\left( aq \right) \right|Pt\left( s \right)\] \[{{E}_{cell}}=0.092V\] when \[\frac{\left[ {{M}^{2+}}\left( aq \right) \right]}{\left[ {{M}^{4+}}\left( aq \right) \right]}={{10}^{x}}\], Given: \[E_{{{M}^{4+}}/{{M}^{2+}}}^{0}=0.151V;2.303\frac{RT}{F}=0.059V\] The value of x is
question_answer13) The electrolysis of acetate solution produces ethane according to reaction - \[2C{{H}_{3}}CO{{O}^{-}}\to {{C}_{2}}{{H}_{6}}\left( g \right)+2C{{O}_{2}}\left( g \right)+2{{e}^{-}}\] The current efficiency of the process is 80%. What volume of gases would be produced at \[27{}^\circ C\] and 740 torr, if the current of 0.5 amp is passed through the solution for 96.45 min?
question_answer14) The cell \[Pt\left| {{H}_{2}}\left( g,0.1bar \right) \right|\] \[\left. {{H}^{+}}\left( aq \right),pH=X \right|\] \[\left| C{{l}^{-}}\left( aq,1M \right) \right|\] \[H{{g}_{2}}C{{l}_{2}}\] \[\left| Hg \right|Pt\], has e.m.f. of 0.5755 V at \[25{}^\circ C\]. The SOP of calomel electrode is \[-0.28V\], then pH of solution will be ?
question_answer15) The chlorate ion can disproportionate in basic solution according to reaction, \[2ClO_{3}^{-}\rightleftharpoons ClO_{2}^{-}+ClO_{4}^{-}\] What is the equilibrium concentration of perchlorate ions forms a solution initially at 0.1 M in chlorate ions at 298 K? [Given: \[E{{{}^\circ }_{\left. ClO_{4}^{-} \right|ClO_{3}^{-}}}=0.36V\] and \[E{{{}^\circ }_{\left. ClO_{3}^{-} \right|ClO_{2}^{-}}}=0.33V\] at 298 K]
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