Which of the following stad(( ;as65eq orr kpno9tements are correct?
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 a dh j-.v4t:zc)t0bvbcell potentials? )htvcb dj4 0va.b z:-t
I.A temperature of 298K
II.A pressure of 100 kPa
III.Solution concentrations of $1\,mol\,dm{-3}$

  Which statement is correctzr8 uxjj :,cx1?

  Which row of the table is correci68bvu *31mi:w h qhpgt for a spontaneous reaction?

  Which statement about electrochemicv eh4fequv3 f/31-jqsal cells is not correct?

  What are the correct products of the reacmu /cdv+4 :yrdtion of nitric acid and magnesium metal? uv+drm/4y:cd

  Which statements about the e 9vg0rd:vgx gu/)0m 7k5x.j wqk 7u;2fertloelectrolysis of 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 tablexxttkg4 *(*wgu 8 l k+ kbgudkj;4lz0; below, contains the correct species that are produced at each electrode during the electrolysis of molten zinc cu zlkwt;(; 4g8k0dg ljtb4gu x*kk+*x hloride?

  Which solution does not produce oxygen at tp *3dj+ 9phd9irb)h ie8g ;pwcv6tfo 6he anode when electrolyzed with inert electroviw )rt*hfh; d6p o+je8pg cbd9 p39i6des?

  Oxygen and water are produced when nitric acid react- noevvb d33tb-g hi(u5+h*eus with potassium manganate(VI bb3+ uhvdg3e-(toe-v5n uhi*I),$KMnO_4$.
$4KMnO_4(aq) + 12HNO_3(aq) \rightarrow 6H_2O(I) + 5O_2(g) + 4KNO_3(aq) + 4Mn(NO_3)_2(aq)$
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 corr:sk0o6q1i xeyhurv p0u6k+ y,ect about 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 reqo p zfb( .):i f80r7vepqwc588nwjcell. The overall reaction taking place in the zq58:fj brnw r 8eop7 efci0wp.vq8)(cell 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 equatik.gp .g+,b dsuon 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 silver isdf0;x 1ap2 54ilys su 2py+z -vz*nlnh incorrect?

  What happens to the 5ml6vj t-ca9pk6 k/o8, nju0p.m zszy$Mn^{3+}_{(aq)}$ ion when it is converted to $MnO_{4(aq)}^-$

  A primary alcohol is heated under reflux with an aqueous st58k9qa cjk yx.af+ns *4a(dtolution of the oxidizing5st*(4kayc+ .ja8ndq 9afkt x agent $KMnO_4$Which of the following is a possible product of this reaction?

  Using the voltaic cell notation given below and the standard electrode potentiab u7xg.n ias0+y 5z)wuve,m9q d d:8sjls, determine the standard cell potential of thuqg:.dba+d78jnx05,)wzv uysmei 9s e 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 momngpa97r llw))hlt(, 9jubu8les of electrons are transferred in the equation for the oxidation of ethanol in the presence of acidified potassium dichromate when balanced with whole numbers?mj l8lp7)ubrgt9 n(w)h,au9 l
$Cr_2O_7^{2-}(aq) + 14H^+(aq) +6e^- \rightarrow 2Cr^{3+}(aq) + 7H_2O(I)$
$CH_3CH_2OH(aq) + H_2O(I) \rightarrow CH_3COOH(aq) + 4H^+(aq) + 4e^-$

  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 electrolysis of molten sodium ch0 t n/wzgf0rmgp73aiu; :s-v lloride. Label the directionv;trwgpm7 0/lg-u f0s in3:az 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 thg i1nqlm.0 4+6vk *nk6xfp:qs pg0n bpe oxidation of a secondary alcohol?

  The diagram below shows a D3qxu8 azr.q, ,0tx yuianiel cell. Zinc is more reactive than copper. When the cell is operating, which statement about the i380z uiryx. ,,q xatquons in the cell is correct?

  What is the reducing aw;w k6lg+bi-e gent in this reaction?
$Zn_{(s)} + 2NO_{3(aq)}^-$ + 4H^+_{(aq)} \rightarrow Zn^{2+}_{(aq)} + 2NO_{2(g)} + 2H_2O_{(I)}$

  The below diagram shows an electrolytic cell. At whiiuy)66q( 0jqoa;o hp xch electrode will bromine form, and woh0o j xyi pq;6(u)a6qhat is the process taking place there?

  The diagram below shows aml--v cz9 *e+ekqj vy6 Daniel cell. Zinc is more reactive than copper. When the spontaneous reaction occurs, which statement about the Daniel cell isz9lkcm+- *6vvy- jq ee correct?

  The equation for the overall reaction in a voltaia x 23hv/ej,imt(* awkc 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 states of sulfur in the following sulfur-cow+n;cfx(ezmro53/lo h. id zm c,h;2rntaining specrco xred(c2; w;nh,/i.l+mf z mzh5o3ies?
$SO_3^{2-}, H_2SO_4, S_8, S_2O_3^{2-}$

  Alkali metals react wisx/f*. p, zqo p*u)yteth water to form 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 nvnox, 1vx93nfc., ;c2ru*ep ex3d whqitrate changes to nitrite ?

Sodium metal may be :qwp1p1iib: pobtained commercially from the electrolysis of molten sodium chloride in a Downs cell. This cell operates as aniq:p bpw:1p1i electrolytic 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 container of wb-.9j-,oxb9qfwuq/g- mnd emolten $CaBr_{2(l)}$ 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 q xfy-,8t :e,fop-d,bkxpy, xredox 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 stand3uoidibc7y ( 1ard 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 write itv q9(ur ,oqt1ss complete balanced chemical equation using the structural formulas of reactants and prs9u qtq(o ,1vroducts.
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 7s*+cr )1b* 4qhbik2 x lrf13if2junqc0e vaopercentage of copper present in a sample of copper (I) oxide. The sample is first dissolved in acidic solix2c v+ lhkbqr1a14n 32f0qi)sebr*j* c fo u7ution 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 reactiof4 s 9+j3d kq,tlr pmwhb,ib44ns involving metals and their aqueous nitrate solution4ijw q,m4+,s d9hlb r4tk3fbps:

	$XNO_3$	$Y(NO_3)_2$	$Z(NO_3)_2$
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 react;5nq jvkc4wqu7 v4:y 5 ibe8d4ukd ml4ions:
$Fe(s) + Cu^{2+}(aq) \rightarrow Fe^{2+}(aq) + Cu(s)$
$Fe(s) + 2Ag^+(aq) \rightarrow Fe^{2+}(aq) + 2Ag(s)$
$Zn(s) + Fe^{2+}(aq) \rightarrow Zn^{2+}(aq) + Fe(s)$
$Cu(s) + 2Ag^+(aq) \rightarrow Cu^{2+}(aq) + 2Ag(s)$

  The equation below shows the reaction between cone hhw7:4wv( d3ta- 0-r.edr3 wmiftnlcentrated sulfuric acid and potassium iodide.hd0nt hd3a(w m-fewre :3rw-vl4 it.7
$8KI(s) + 5H_2SO_4(aq) \rightarrow 4K_2SO_4(aq) + 4l2(g) + H_2S(g) + 4H_2O(l)$
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 equations0-f 37v1npj kc+ ggs n gq:*i6vvo.fa amay6;m:
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