Which of the following statements are correctt f(xnkxj 3)g*ytw3k 4cm6zpi twc620?
I.Voltaic cells convert chemical energy into electrical energy
II.Electrolytic cells convert electrical energy into chemical energy
III.Electrolytic cells require a salt bridge

  Which of the following are the standard conditions for standard celttvs1 ;b- 4.r4w*zsdh j( ozerld(la-l potentials?z-ts*sh;jl . 4(z4 va twdodb(rl1e-r
I.A temperature of 298K
II.A pressure of 100 kPa
III.Solution concentrations of $1\,mol\,dm{-3}$

  Which statement is correct?5zp(4a ofv/unjbq x*jvy *s*1

  Which row of the table is dd i/xka d(7xvqhpx u/h3 7o(ye9jecp3w. ;n8correct for a spontaneous reaction?

  Which statement about electrochemical cells is 1 dlajxg0 9( lwk 2e,j+2wswaanot correct?

  What are the correct products of th9nvzl8 bn k5+ye reaction of nitric acid and magnesium metalz y5nb9l+8 vkn?

  Which statements about the electrolysis of dhaa+6w gr(-j molten aluminium oxide are correct?
I. Aluminium ions gain electrons at the cathode
II. Oxide ions lose electrons at the cathode
III. The cathode is the site of reduction in this cell

  Which row, indicated in the table cu 8*lrd*l7qvbelow, contains the correct species that are produced at each elec* dvqcu* l7r8ltrode during the electrolysis of molten zinc chloride?

  Which solution does not yx *:1 s1q9yms3yv6umo8xdyi v;tcr 4produce oxygen at the anode when electrolyzed with inert electro t3c4q9imsy x8 vov:u11x;y6mdys r* ydes?

  Oxygen and water are p*5pv 1or/o67b.6xpor zfeznh -1 cnhm roduced when nitric acid reacts with potassium manganate(VII),no h c-h vr1 fpm76. p1e/x6zzon5*obr$KMnO_4$.
$4KMnO_4(aq) + 12HNO_3(aq) \rightarrow 6H_2O(I) + 5O_2(g) + 4KNO_3(aq) + 4Mn(NO_3)_2(aq)$
1.Define reduction in terms of electron transfer.
2.State the oxidation state of manganese in $KMnO_4$ and in $Mn(NO_3)_2$.In $KMnO_4$:X= ----待选择----+-   , In $Mn(NO_3)_2$:X= ----待选择----+-   
3.Identify which species has been oxidized in this reaction and specify the change in oxidation state it has undergone.

  Which statements are correct about an electrolytic cell?z nh.-t0h.hdxg:rm o5
I. An external power supply is used to drive a non-spontaneous process
II.Oxidation occurs at the positive electrode in the cell
III.The cell could be used to extract a reactive metal from its molten salt

  The diagram below showsa vg:+h, uxt:m a voltaic cell. The overall reaction taking place in the ce:tx, huagv:m+ll is:
$Mg(s) + Pb^{2+}(aq) \rightarrow Pb(s) + Mg^{2+}(aq)$


Which statement is correct for the magnesium half cell?

  What is the balanced chem)9xm w6o 0a/mhfjm +lhical equation and $E^{\theta}$ cell for the spontaneous reaction between the following half-cells?
$Pb^{2+}(aq) + 2e^- \rightarrow Pb(s)$ -0.13V
$Cu^{2+}(aq) + 2e^- \rightarrow Cu(s)$ +0.34V

  Which statement about electroplating an object with w e5ar6;9yc.voft p -csilver is incorrect?

  What happens to the x3y,:nji xgb0$Mn^{3+}_{(aq)}$ ion when it is converted to $MnO_{4(aq)}^-$

  A primary alcohol is heated under reflux 5 bbl6 qypx+a5esu71q- yxns8 with an aqueous solution of the oxidiziny55 +qqlxyes n 8x 16s-ba7bpug agent $KMnO_4$Which of the following is a possible product of this reaction?

  Using the voltaic cell notation given below and thdpb wj;9msfve1 nx88bi.b a -)e standard electrode potentials, determine -b.n9ea ); sd bxbvjm p18i8wfthe standard cell potential of the cell,$E^{\Theta}$.
$Pb(s) | Pb^{2+}(aq) || Ag^+(aq) | Ag(s)$
$Ag^+(aq) + e^- \rightarrow Ag(s)$ +0.80V
$Pb^{2+}(aq) 2e^- \rightarrow Pb(s)$ -0.13V

  Using the following half reactions, how many moles of electrons are traobzsxaii0u9xu s) cd u9equww2*10:+nsferred in the equation for the oxidation of ethanol in the presence of acidified potassium dich* 0u2wxz1u)0bsa w+9iui xceqodsu :9romate when balanced with whole numbers?
$Cr_2O_7^{2-}(aq) + 14H^+(aq) +6e^- \rightarrow 2Cr^{3+}(aq) + 7H_2O(I)$
$CH_3CH_2OH(aq) + H_2O(I) \rightarrow CH_3COOH(aq) + 4H^+(aq) + 4e^-$

  Electrolysis of $Cu^{2+}$ using a current of 1A for 10s produces x mol of Cu metal.
If Q= It, how many moles of Cu metal is produced if $Cu^+$ is electrolyzed under the same conditions?

1.Draw an electrolytic cell for the electrolys6n0laz s2uz.c3i,u 4 pw4ug nais of molten sodium chloride. Label thegwuzi.u6 u n4a lcsz0,p 32an4 direction of electron flow and the polarity of the electrodes.
2. 1.Deduce the major products if dilute aqueous sodium chloride was electrolysed instead.
2.Deduce the major products if concentrated aqueous sodium chloride was electrolysed instead.

  Which of the below reactions shows the oxidation of a secondaryjguva 4* l:hb4/ mlqj- alcohol?

  The diagram below shows a Daniel cell. Zinc is more redx4+dg4e/ +ipeevjj*active than copper. When the cell is operating, which statemxdee4i+gjjd v p+e/*4ent about the ions in the cell is correct?

  What is the reducing agent in this reactiqib;ve nx n+3)m).cvgq , q;o h;9kbmyon?
$Zn_{(s)} + 2NO_{3(aq)}^-$ + 4H^+_{(aq)} \rightarrow Zn^{2+}_{(aq)} + 2NO_{2(g)} + 2H_2O_{(I)}$

  The below diagram show.fm)vrn9e/ pm s an electrolytic cell. At which electrode will bromine form, a. nvfmp) /9ermnd what is the process taking place there?

  The diagram below shows a Daniel cell. Zinc is more reactivg68km)9q q zp*kp bj-ve than copper. When the spontaneous reaction occurs, which statement about the Daniel cell is correct? 9pvbqzpmq6gk*j8 k)-

  The equation for the overall reaction in a voltaic cell is: v 7;gb wp 8mh6ac3q/a7sdfo8* 6kdjce
$Cu(s) + 2Ag^+(aq) \rightarrow Cu^{2+}(aq) + 2Ag(s)$
Which statements are correct for this cell?
I. Electrons flow from the copper electrode to the silver electrode
II. Silver ions are reduced in the reaction
III. The copper anode will become smaller in size as the reaction proceeds

  What are the respective oxidation states of suh z1mbqxl d77:lfur in the following sulfur-containing:dbl 1zx7mqh7 species?
$SO_3^{2-}, H_2SO_4, S_8, S_2O_3^{2-}$

  Alkali metals react with water to iv, sb*p hnc:dt65 yh c89a be783yxhsform metal hydroxide and hydrogen gas.
1.Write a balanced equation between sodium and water.
2.Explain why this reaction is considered as a redox reaction.
3.3 other alkali metals W, X and Y also react with water.
Based on the following observations, arrange the metals in order, starting from the weakest oxidizing agent. Explain your answer. ----待选择----XYW $\lt$ ----待选择----XYW $\lt$ ----待选择----XYW $\lt$

Meta	Observations
W	Slow reaction with water
X	Vigorous reaction with water
Y	Fast reaction with water

  What happens to nitrogen when nitrate changes to nitrite 3rfq8 t ;:c i/;6xkqxkx5ugc7cn;lov?

Sodium metal may be obtained commercially ina6fre l)g,e n/bj.sl3ky0bx15j1 p from the electrolysis of molten sodium chloride in a Downs cell. This cell operates as an electrolytic cgflpk 0yb6 jxan1 ne1 53bjls.r,i)/eell.
1.Describe, using a diagram, the essential components of this electrolytic cell.
2.Suggest why molten sodium metal may be collected from the top of this type of cell.
3.Describe two ways in which current is conducted in an electrolytic cell.

  A battery is added to a container w 9bwtx8*t1 l ygrm6(nof molten $CaBr_{2(l)}$ to create an electrolytic cell, as shown in the diagram below.



1. 1Use section 24 (Section 19- 2025 Syllabus) of your data booklet to identify and write the oxidation and reduction half-reactions.
2.Label the anode and cathode on the diagram above.
3.On the diagram above, label the electrode where calcium metal $(Ca_{(s)})$will appear.
2.A different electrochemical cell is shown below. One half-cell contains a lead metal electrode immersed in 1.0 M $Pb(NO3)_2$ solution. A standard electrode potential table is also shown for elements X, Y, and Z.

Elements	Electrode potential
$X^{2+}_{(aq)} + 2e^- \rightarrow X_{(s)}$	$E^{\Theta}$=-1.18V
$Y^+_{(aq)} + 1e^- \rightarrow Y_{(s)}$	$E^{\Theta}$=-0.45V
$Z^{2+}_{(aq)} + 2e^- \rightarrow Z_{(s)}$	$E^{\Theta}$=+0.34V

1.Label the left half-cell of the diagram with the metal that will produce the highest cell potential.
2.Draw an arrow on the diagram indicating the direction of the flow of electrons.
3.Consult section 24 (Section 19- 2025 Syllabus) in your data booklet to calculate the standard cell potential for the diagrammed cell.  V
4.Use metals X, Y, and Z combined with aqueous chloride solutions of metals X, Y, and Z, and write a balanced equation for a reaction that will proceed spontaneously.

  Consider the following redo zn :eti*0ju-rq 5gb0if0v bg1zgzh +*x reaction:
$Cr_2O_7^{2-}(aq) + 14H^+(aq) + 6Ag(s) \rightarrow 2Cr^{3+}(aq) + 7H_2O(l) + 6Ag^+(aq)$
1. 1.Using section 24 (Section 19- 2025 Syllabus) of the data booklet, calculate the standard cell potential.  V
2.Predict, with a reason, whether this reaction is spontaneous or not.
2.Using sections 1 and 2 of the data booklet, calculate the standard Gibbs free energy change in $kJ\,mol^{-1}$.
The standard entropy change for this reaction is $508J\,K^{-1}\,mol^{-1}$
3.Using section 1 of the data booklet, calculate the standard enthalpy change for this reaction in $kJ\,mol^{-1}$.
$\Delta G^{\Theta}$=  $kJ\,mol^{-1}$, $\Delta H^{\Theta}$=  $kJ\,mol^{-1}$

  The Daniell Cell is a galvanic cell with a standard cell potential of 1.10n+31gq sa3 onkp0m* 1nf1r(lw(q eep hV.
$Cu^{2+}(aq) + Zn(s) \rightarrow Cu(s) + Zn^{2+}(aq)$
1. 1.Define standard electrode potential.
2.List the features of a standard hydrogen electrode (SHE).
Suppose the SHE is replaced by a MMSE reference electrode with a standard electrode potential of 0.64V.
2. 1.Using section 24 (Section 19- 2025 Syllabus) of the data booklet, calculate the new electrode potentials.Cu(s):  V, Zn(s):  V
2.Using your answers to (b)(i), calculate the new cell potential and comment on this value.$E_{cell}$=  V

For each reaction described below, specify its type and write its complete bd .o4gm dmb:tq3(awe3alanced chemical eqmtg.o(3dw4d bq :m3eauation using the structural formulas of reactants and products.
1.Formation of butane from but-2-ene.
2.Formation of but-2-one from butan-2-ol.

  Titration technique can be used to determine the percentage of copper present i)zmn vya:gnf hxl9/ 14n a sample of copper (I) oxide. The sample is fivznl/gayx1 )9:nh4 mf rst dissolved in acidic solution and $Cu^+$ ions are formed. The resulting solution is then titrated against a standard solution of potassium manganate (VII),$KMnO_{4}$. In acidic solution,$MnO^-_4$ reacts with $Cu^+$ to form $Mn^{2+}$ and $Cu^{2+}$ ions.

Titre	1	2	3
Initial burette reading/$cm^3$	2.00	24.70	5.00
Final burette reading/$cm^3$	25.80	48.30	30.60

Mass of copper oxide (I) sample/g 0.7751
Concentration of $KMnO_{4}$ solution/$mol\,dm^{-3}$ $2.375\times10^{-2}$
1.Using Section 24 (Section 19- 2025 Syllabus)of the Data Booklet, write the equation of the redox reaction.
2.Define reducing agent and specify the reducing agent in the reaction.
3.Calculate the number of moles of $MnO^-_4$ that reacted with $Cu^+$.  $cm^3$
4.Deduce the percentage by mass of Cu present in the sample.  %
Important note: The section numbers mentioned in the video solution are specific to the 2024 syllabus.
You can refer to the question stem to find the section numbers in the 2025 syllabus.

  Consider the following reactions i s(2x:ogd) ,tw 7svylnnvolving metals and their aqueous nitrate solutions: s7 dnwtg2:y)slv o (x,

	$XNO_3$	$Y(NO_3)_2$	$Z(NO_3)_2$
Metal X		No reaction	No reaction
Metal Y	Grey solid of metal X observed		No reaction
Metal Z	Grey solid of metal X observed	Pink solid of metal Y observed

Choose the correct order of the metals from the strongest oxidizing agent to the weakest?

  Consider the following r3uxd v vr * zq(e7a5q5-rb5kyreactions:
$Fe(s) + Cu^{2+}(aq) \rightarrow Fe^{2+}(aq) + Cu(s)$
$Fe(s) + 2Ag^+(aq) \rightarrow Fe^{2+}(aq) + 2Ag(s)$
$Zn(s) + Fe^{2+}(aq) \rightarrow Zn^{2+}(aq) + Fe(s)$
$Cu(s) + 2Ag^+(aq) \rightarrow Cu^{2+}(aq) + 2Ag(s)$

  The equation below shows the reaction between concentrated sulfuric acid and 290irco4bk 7d xh(hl.,loxvfpotassium iodidehorv.f4c2xhd, bx97i olk(0l .
$8KI(s) + 5H_2SO_4(aq) \rightarrow 4K_2SO_4(aq) + 4l2(g) + H_2S(g) + 4H_2O(l)$
1.State the oxidation state of sulfur in $H_2SO_4$ and $4H_2S$.In $H_2SO_4$, x= ----待选择----+-   , in $4H_2S$, x= ----待选择----+-   
2.Write the half equations for the oxidation and reduction reactions.
3.Define oxidizing agent in terms of electrons.
4.Identify the oxidizing agent in the equation.

  Consider the following equatiou bn:pr9 ea0;; .jx yd1e0vah ovm6d0 7sml9twns:
Equation 1:
$2ClO_3^-(aq) + I_2(aq) \rightarrow Cl_2(aq) + 2IO_3^-(aq)$
Equation 2:
$ Cl_2(aq) + 2NaOH(aq) \rightarrow NaCl(aq) + NaClO(aq) + H_2O(l)$
Which statements about these reactions is/are not correct?
I.Iodine is reduced in equation 1
II.Chlorine is reduced only in equation 1
III.Chlorine is oxidized and reduced in equation 2