Which of the following statements are correctrzh8-;oq7 uj r?
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 conditionatd -b c:,9,rf*t jmu,2qki5gynz:m bz,iu8 js for standard cell potentials?j8cf:z :nk ,9rm u,, b-*g,5id2tizbmayujtq
I.A temperature of 298K
II.A pressure of 100 kPa
III.Solution concentrations of $1\,mol\,dm{-3}$

  Which statement is correcw66ihj7nn kf 5gb6o o5t?

  Which row of the table is correct for a spon(lolyc* f7bh,taneous reaction?

  Which statement about electrochjr l2e:j.i idamif:1jys)q, 8 8c hg:gemical cells is not correct?

  What are the correct products of the reac/h,iy : hwf 4jk+ v3co.mxx ff(jacz.-tion of nitric acid and magnesium metal?,f hm x../-4occvi jykzha(3w+jx:f f

  Which statements about the electrolysis of molten aluminium oxide are +-iubrr 88 utmcorrect?
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 be l )vmds(gpduqz7:o7, low, contains the correct species that are produced at each electrode during the elect 7q7, z(vmupd dg:ols)rolysis of molten zinc chloride?

  Which solution does not produce oxywd) t6q1.moziu0wm(j mi*eu5:f.la j gen at the anode when electrolyzed with inert electr u .)i a1j .zwm5f tqu6owm:d0jm(ie*lodes?

  Oxygen and water are produced when nitric acid reacts with potassi9fh/gqco7stch:u75(t hdw; ut* ;rn lum manganate(VII), ; (;ug7n7t/r*tc hhtf5o :cwuhlqsd9 $KMnO_4$.
$4KMnO_4(aq) + 12HNO_3(aq) \rightarrow 6H_2O(I) + 5O_2(g) + 4KNO_3(aq) + 4Mn(NO_3)_2(aq)$
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 aboutyuse4t-g xk * a*kuz1+ 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. The overall reaction taking pluh ton;r a*.m5sxr 60 ierd+;yace in the cell is: xe0.*5 6nmrrht;+;r iusdyoa
$Mg(s) + Pb^{2+}(aq) \rightarrow Pb(s) + Mg^{2+}(aq)$


Which statement is correct for the magnesium half cell?

  What is the balanced5ymv2fr8s8 hr2ev 7 fk chemical 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 electroplati lvj- +1a r ,qy1pol:t0fye g)))sdsjing an object with silver is incorrect?

  What happens to the 1qvctlvm ct-28+7 fnp1- rhnz$Mn^{3+}_{(aq)}$ ion when it is converted to $MnO_{4(aq)}^-$

  A primary alcohol is heau8vh0daeb,x soa 6z6(29kitha wt2 p/ted under reflux with an aqueous solution of the oxidizing agent bv6d a ohh2a2/ptwk(i x9z, a6eus80 t$KMnO_4$Which of the following is a possible product of this reaction?

  Using the voltaic cell notation given below and the standard ;p3 (zwf .v78m xkoeahelectrode potentials, deapvwfkox 3 8e.m7(zh;termine the 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 mippn (.q:gnsmd43a6 .x9q fb jany moles of electrons are transferred in the equation for the oxidation of ethanol in the i dx94fpq.(6bm 3sna: j.gqpnpresence 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 v(mh 8va dybo6l1h23 3o- jcwrcell for the electrolysis of molten sodium chloride. Label the direction d vhlma(-3 wrhcyo38j2b16v o 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 secondary alcohol92pw;yrsni bwf48 id sq.73dg?

  The diagram below shows a Daniel cell. Zinc is more reatwhiq4 ol.t-ia73y e3 ctive than copper. When the cell is operating, which statement about the ions in the cell is correc-i74 yqo.3wti3hea tlt?

  What is the reducing agent (q4v5n.bru)1keu m mxin 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 which electrtfkxqt+13 qv ne8s jc2f5y2n8ode will bromine form, and what i+nf15n 8 jqt2yxc 2stq83v kefs the process taking place there?

  The diagram below shows a Daniel c m.:o)wfyjhb+lh/3x,pgsw/ bds u 2g6ell. Zinc is more reactive than copper. When the spontaneous reaction occurs, which statement about the Daniel ce3gy/m.obdswbflg2ux:+ )h sj6/w ,hpll is correct?

  The equation for the overall ir b0 lpctv;28wvq29 nreaction 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 states of sulfur in the ,aoj h*a0z 8/xlz :umofollowing sulfur-containing spec a*m j/xao:o z0lh8zu,ies?
$SO_3^{2-}, H_2SO_4, S_8, S_2O_3^{2-}$

  Alkali metals react with wate+y*-l (xfvwt gr 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 nitrate changes rv3 jgf g/41aj;ry7sd to nitrite ?

Sodium metal may be obtained commercialeo)0iwxicb :wvpprr,g8 2w9,ly from the electrolysis of molten sodium chloride in a Downs cell. This cell operates as an electrolytic celew0rp:2cwor ii)p ,xb,wv9g8l.
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 contaur *w0cz) fn,oiner 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 followingtb(9.h fn8djhu,r( szw 3 3fre redox 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 gat0fyr2 sro**a 4s;dnl lvanic cell 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 typu 7ey8pnps4n wnc)8z: e and write its complete balanced chemical equation using the structural formulas of reactants )7peuc84snz: 8n nwpy 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 presabbx;t tj*2-yp 9q)xp ent in a sample of copper (I) q yaxbp;2t*p)bt xj9- oxide. 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 invf:ma1* jdbf-k d)szbs- p3u :( plpnp5olving metals and their aqueous nitrate solut *51-3l fjzsm pu)sap(p-fk:d: bpdnbions:

	$XNO_3$	$Y(NO_3)_2$	$Z(NO_3)_2$
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 reactions kx6vga)y, zd1:
$Fe(s) + Cu^{2+}(aq) \rightarrow Fe^{2+}(aq) + Cu(s)$
$Fe(s) + 2Ag^+(aq) \rightarrow Fe^{2+}(aq) + 2Ag(s)$
$Zn(s) + Fe^{2+}(aq) \rightarrow Zn^{2+}(aq) + Fe(s)$
$Cu(s) + 2Ag^+(aq) \rightarrow Cu^{2+}(aq) + 2Ag(s)$

  The equation below shows the reaction betweeni(i3 4)rza xn :f/eabi concentrated sulfuric acid and potasi3 bx ir(a:4 )eaf/inzsium iodide.
$8KI(s) + 5H_2SO_4(aq) \rightarrow 4K_2SO_4(aq) + 4l2(g) + H_2S(g) + 4H_2O(l)$
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 equations5e;uo t;l+;i;l mkmvm :
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