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First Year Chemistry Electrochemistry


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(d)Calculatetheoxidationnumbersoftheelementsunderlinedinthefollowingcompounds.(ii)Na2CO3(d) Calculate the oxidation numbers of the elements underlined in the following compounds.(ii) \mathrm{Na}_{2} \mathrm{CO}_{3}

9. \mathrm{lg} equivalent weight of \mathrm{Al} is equal to(a) 9 \mathrm{~g} (b) 27 \mathrm{~g} (c) 54 \mathrm{~g} (d) \mathrm{lg}
9.  \mathrm{lg}  equivalent weight of  \mathrm{Al}  is equal to(a)  9 \mathrm{~g} (b)  27 \mathrm{~g} (c)  54 \mathrm{~g} (d)  \mathrm{lg}

9.lgequivalentweightofAlisequalto(a)9 g(b)27 g(c)54 g(d)lg9. \mathrm{lg} equivalent weight of \mathrm{Al} is equal to(a) 9 \mathrm{~g} (b) 27 \mathrm{~g} (c) 54 \mathrm{~g} (d) \mathrm{lg}

(b) Balance the following equations by oxidation number method(iii) \mathrm{Br}_{2}+\mathrm{NaOH} \rightarrow \mathrm{NaBr}+\mathrm{NaBrO}_{3}+\mathrm{H}_{2} \mathrm{O}
(b) Balance the following equations by oxidation number method(iii)  \mathrm{Br}_{2}+\mathrm{NaOH} \rightarrow \mathrm{NaBr}+\mathrm{NaBrO}_{3}+\mathrm{H}_{2} \mathrm{O}

(b)Balancethefollowingequationsbyoxidationnumbermethod(iii)Br2+NaOHNaBr+NaBrO3+H2O(b) Balance the following equations by oxidation number method(iii) \mathrm{Br}_{2}+\mathrm{NaOH} \rightarrow \mathrm{NaBr}+\mathrm{NaBrO}_{3}+\mathrm{H}_{2} \mathrm{O}

(b) Balance the following ionic equations by ion-electron method.(iv) \mathrm{Cu}+\mathrm{NO}_{3}^{1-} \rightarrow \mathrm{Cu}^{2+}+2 \mathrm{NO}_{2}
(b) Balance the following ionic equations by ion-electron method.(iv)  \mathrm{Cu}+\mathrm{NO}_{3}^{1-} \rightarrow \mathrm{Cu}^{2+}+2 \mathrm{NO}_{2}

(b)Balancethefollowingionicequationsbyionelectronmethod.(iv)Cu+NO31Cu2++2NO2(b) Balance the following ionic equations by ion-electron method.(iv) \mathrm{Cu}+\mathrm{NO}_{3}^{1-} \rightarrow \mathrm{Cu}^{2+}+2 \mathrm{NO}_{2}

Q.1 Multiple choice questions.(v) If a strip of Cu metal is placed in a solution of \mathrm{FeSO}_{4} :(a) Cu will be deposited(b) Fe is precipitated out(c) Cu and Fe both dissolve(d) No reaction take place
Q.1 Multiple choice questions.(v) If a strip of Cu metal is placed in a solution of  \mathrm{FeSO}_{4}  :(a) Cu will be deposited(b) Fe is precipitated out(c) Cu and Fe both dissolve(d) No reaction take place

Q.1Multiplechoicequestions.(v)IfastripofCumetalisplacedinasolutionofFeSO4:(a)Cuwillbedeposited(b)Feisprecipitatedout(c)CuandFebothdissolve(d)NoreactiontakeplaceQ.1 Multiple choice questions.(v) If a strip of Cu metal is placed in a solution of \mathrm{FeSO}_{4} :(a) Cu will be deposited(b) Fe is precipitated out(c) Cu and Fe both dissolve(d) No reaction take place

21. In electroplating of silver from where \mathrm{Ag}^{+} ions come and where they deposit?
21. In electroplating of silver from where  \mathrm{Ag}^{+} ions come and where they deposit?

21.InelectroplatingofsilverfromwhereAg+ionscomeandwheretheydeposit?21. In electroplating of silver from where \mathrm{Ag}^{+} ions come and where they deposit?

(b) Balance the following equations by oxidation number method(ix) \mathrm{NaCl}+\mathrm{H}_{2} \mathrm{SO}_{4}+\mathrm{MnO}_{2} \rightarrow \mathrm{Na}_{2} \mathrm{SO}_{4}+\mathrm{MnSO}_{4}+\mathrm{H}_{2} \mathrm{O}+\mathrm{Cl}_{2}
(b) Balance the following equations by oxidation number method(ix)  \mathrm{NaCl}+\mathrm{H}_{2} \mathrm{SO}_{4}+\mathrm{MnO}_{2} \rightarrow \mathrm{Na}_{2} \mathrm{SO}_{4}+\mathrm{MnSO}_{4}+\mathrm{H}_{2} \mathrm{O}+\mathrm{Cl}_{2}

(b)Balancethefollowingequationsbyoxidationnumbermethod(ix)NaCl+H2SO4+MnO2Na2SO4+MnSO4+H2O+Cl2(b) Balance the following equations by oxidation number method(ix) \mathrm{NaCl}+\mathrm{H}_{2} \mathrm{SO}_{4}+\mathrm{MnO}_{2} \rightarrow \mathrm{Na}_{2} \mathrm{SO}_{4}+\mathrm{MnSO}_{4}+\mathrm{H}_{2} \mathrm{O}+\mathrm{Cl}_{2}

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