Which of the following statements are corr1ndpnpn 4.axz95 t ea7ect?
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 t9ob8d t3* wpsthe standard conditions for standard cell potentials? *tws8 pb d9o3t
I.A temperature of 298K
II.A pressure of 100 kPa
III.Solution concentrations of $1\,mol\,dm{-3}$

  Which statement is correu/de ts5 jvtxv7v l02 tx*.xa2wd0 gi7ct?

  Which row of the table is co 1qzet t*1*deb:h6o wlrrect for a spontaneous reaction?

  Which statement about electrochemical cellq fid4 ye9p kns 97zgxx.wz+48s is not correct?

  What are the correct n8gt-h*2cr:4ezerhmg3h c mmax0i, :products of the reaction of nitric acid and magnesium metal8zg- 3rt4mg hm,c0:ch :2meirxn * hea?

  Which statements about the electrolysis o+:ss/ixy)g8g9v l d bdf 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 i6jq(-tm 9njw dn the table below, contains the correct species that are produced at each electrode during the electrolysis ofwn9 j6j(m qd-t molten zinc chloride?

  Which solution does not produce oxygen at the anode when .cj et8cf ttj: omda7h h:;dz8d vhg4/0o .p,celectrolyzed with inert eleccaf .;0h:,h d47odzhm8ot8/t v.jpcdgce t :jtrodes?

  Oxygen and water are produced when nitric acid reacts wit kcpf:.fl7 j94x .5hj nrp2jvqh potassium manganate(VIIkcj.ph2fjl9x.4 vp7 nq :5fjr),$KMnO_4$.
$4KMnO_4(aq) + 12HNO_3(aq) \rightarrow 6H_2O(I) + 5O_2(g) + 4KNO_3(aq) + 4Mn(NO_3)_2(aq)$
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 aw)hlryb4uthvicg r0a y0 ; j+8:pbs5ebb :9p8 bout an electrolytic cell?
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 shows a voltaic cell.*re j pp55o-pe The overall reaction taking place in the cell5o -jrpp5p ee* 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 chemical equati;4/bm0 jkmqus on 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 elerj (vttw-*fz 3ctroplating an object with silver is incorrect?

  What happens to the )ltcl2- qu:f ri u0(so5ki8l .(xyviou6d2se$Mn^{3+}_{(aq)}$ ion when it is converted to $MnO_{4(aq)}^-$

  A primary alcohol is heated u b1saw i7j37) pw1u jrobi2h+3(cw*-i decoo under reflux with an aqueous solution of the oxidizingujs abio )e7o (h* i31-7uibc2w3c p d1+rwowj agent $KMnO_4$Which of the following is a possible product of this reaction?

  Using the voltaic cell notat2kgr0sj 8x9ll: o,k uqion given below and the standard electrode potentials, determine the standard cegq klj:sl ,ku982r0oxll 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 ar8(t1 eq 0pitqpp,p-3qjv l aa7e transferred in the e (0-aqp pp3vtiq1 qp l8etaj,7quation for the oxidation of ethanol in the presence of acidified potassium dichromate 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 ce/lbs9/8uz5: qpz mqlc0ycuhy7:, d ojll for the electrolysis of molten sodium chloride. Label the direction of electron flow and the polarity of the electr ul: j0 q/yd8/m9,7s lhcb:yoqzzu5cpodes.
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 secondaryc t(v 1d7t1teci: ;,zo9acz jyr;l*tf alcohol?

  The diagram below shows a Daniel cell. Zinc is more reactive than copper. Whek +h:fo(tf*r jn the cell is operating, which statement about th(:hffj t*+rok e ions in the cell is correct?

  What is the reducing m ltb99yo/pp 8agent in this reaction?
$Zn_{(s)} + 2NO_{3(aq)}^-$ + 4H^+_{(aq)} \rightarrow Zn^{2+}_{(aq)} + 2NO_{2(g)} + 2H_2O_{(I)}$

  The below diagram show/h 3 p/wfma((y dcmk6*znl.mps an electrolytic cell. At which electrode will bromine form, and what is the process taking pk fzwn (ml*pah 6/m(mcd yp./3lace there?

  The diagram below shows a fs pcwkre/3 t3hb.2 *nqu+,vwDaniel cell. Zinc is more reactive than copper. When the spontaneous reaction occurs, which statement about the Daniel cell is correcu. rn3tbpq e,+wfsw3*/h 2 cvkt?

  The equation for the overall reac xjmzn.)cm/ek+j6 xw4 tion in a voltaic cell is:
$Cu(s) + 2Ag^+(aq) \rightarrow Cu^{2+}(aq) + 2Ag(s)$
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 sb2zftz dr1 .y,tates of sulfur in the following sulfur-containizdtz , b1.yrf2ng species?
$SO_3^{2-}, H_2SO_4, S_8, S_2O_3^{2-}$

  Alkali metals react with water to form mk 2ch1u7il5qx etal 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 nitriyzs;r yr.w rb1 cg+f7;te ?

Sodium metal may be obtained commerciaw qb j.)r a-oey554hhhlly from the electrolysis of molten sodium chloride in a Downs cell. This cell operates as an ela -h o hqre55j)yh4.bwectrolytic cell.
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 containet-j15pl;ec se2c( bgo r of 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 z cfqlr0*kpx5ch2 9( dredox 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 cel4ycjhu0o /4a (*9 bpeir 3owf *fu6mnyl with a standard cell potential of 1.10V.
$Cu^{2+}(aq) + Zn(s) \rightarrow Cu(s) + Zn^{2+}(aq)$
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 wrso7+hp, q.,exo 5oeql ite its complete balanced chemical o75oqeo, e.xl+s qp ,hequation 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 deterq/px73b27 5kk xtk t tb yp3c;fjt9-cumine the percentage of copper present in a sample of copper (I) oxide. kp9x7p 3t3k7 -ccft2btx y;kjtq/b5u The sample is first 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 involving metals and their aqueous nitbw*gsc.h/, *x fq7-wtp2 ed2;y1bevs: tl ulzrate solutionsq:dzbcy.te - v2g; w*wt ,/u 27e blls1spfhx*:

	$XNO_3$	$Y(NO_3)_2$	$Z(NO_3)_2$
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 reactw jc6uf; b:.ccions:
$Fe(s) + Cu^{2+}(aq) \rightarrow Fe^{2+}(aq) + Cu(s)$
$Fe(s) + 2Ag^+(aq) \rightarrow Fe^{2+}(aq) + 2Ag(s)$
$Zn(s) + Fe^{2+}(aq) \rightarrow Zn^{2+}(aq) + Fe(s)$
$Cu(s) + 2Ag^+(aq) \rightarrow Cu^{2+}(aq) + 2Ag(s)$

  The equation below shows the reaction b l r64/l izpq.m1l+pi )dz5k/vsa1oe netween concentrated sulfuric acid and potassium iodide.m r z1nz65qdaki. 4 vpoe/lisl+l1/p)
$8KI(s) + 5H_2SO_4(aq) \rightarrow 4K_2SO_4(aq) + 4l2(g) + H_2S(g) + 4H_2O(l)$
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 x hbh 2u/xa,d:9cd c.,7mvhgtequations:
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