Which of the following sv +6guc..-bh.ynhl g z;pza; ctatements 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 condip7-- sjtbduhk44 b*j ptions for standard cell potentials? 7j4pdps 4uhj-k*- bt b
I.A temperature of 298K
II.A pressure of 100 kPa
III.Solution concentrations of $1\,mol\,dm{-3}$

  Which statement is correu*wjl 7t7 )9rylq7afp ct?

  Which row of the tablh pz49kz(,qh/ktu m-g e is correct for a spontaneous reaction?

  Which statement about electrochemical cells is n4k b)v3rn e w6vo9h6caot correct?

  What are the correct products of the reactgmz.( qy ;+voyal m96d 7zit5xion of nitric acid and magnesium metal?6y7t gdz.il(v q;ao9m 5yxzm+

  Which statements about the electrolysis of molten aluminium oxide are cory+ikusa4 9/i sq6)3 xtju zd5drect?
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 below, contayt4vx-x* hgsg(w1 q 9nins the correct species that are produced at each electrode during the electrolysis of moltengv qwstg(h-yn914 *x x zinc chloride?

  Which solution does not produce oxygen at the anode when electrolyzed wyo74 g o.ak3hbith inert elecy gah o4k7.bo3trodes?

  Oxygen and water are produced when nitric acid reacts with potassium k6.r l -lsz/rbmanganate(VI-lb/zk6 .lr srI),$KMnO_4$.
$4KMnO_4(aq) + 12HNO_3(aq) \rightarrow 6H_2O(I) + 5O_2(g) + 4KNO_3(aq) + 4Mn(NO_3)_2(aq)$
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 abom3h*g 5 hesw4.6mlg yl-s2ecaut 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 dcjp9i78deqtu,df), x) +n* su ww6ewtaking place in the cell is: )*cdwtn6wpjued+ 8edx,q )fs9,7uwi
$Mg(s) + Pb^{2+}(aq) \rightarrow Pb(s) + Mg^{2+}(aq)$


Which statement is correct for the magnesium half cell?

  What is the balanced chemical equa4 qwyhj( cj1k1tion 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 electroplatiql5pkv g(ojgfc d 7-(s+lp. u1ng an object with silver is incorrect?

  What happens to the vx;)4y ab0 eyv$Mn^{3+}_{(aq)}$ ion when it is converted to $MnO_{4(aq)}^-$

  A primary alcohol is h15w3 alwiwm -p7sbv--rju xu+eated under reflux with an aqueous solution of the oxidizing a+-5aw 1lwiujvb37 x-spu rw -mgent $KMnO_4$Which of the following is a possible product of this reaction?

  Using the voltaic cell nz0 s.f90fu)3u cpe1otgtg u+ pr7 rds-otation given below and the standard electrode potentialsc+pf03ezt 9su r- 7 tsg).oug1rdup0f, determine 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 many moles of electrons7ozz2yfbfzd47 jh ) o4 are transferred in the equation for the oxidation of ethanol in the presence of acidified potassium dichromate when balanced with wholeb yfz4 z7dfh7ojoz42) 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 cd -c ;4mnj9ux +b0aag- rka,wsell for the electrolysis of molten sodium chloride. Label the direction of electron flow and the polarity of the electrobsm0k-aanjwgucd - +a;49,xr des.
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 reac4fgz 1/ny;rmpc2 rv6 gtions shows the oxidation of a secondary alcohol?

  The diagram below shows a Daniel cell. Zinc is more react3trde:o(h1 jy.fi re1 ive than copper. When the cell is operating, which statement about the d ej1:.rye(ohfir1 t3ions in the cell is correct?

  What is the reducing agent in this rea oga -kv: h:7ybazd6i3+b0nbrction?
$Zn_{(s)} + 2NO_{3(aq)}^-$ + 4H^+_{(aq)} \rightarrow Zn^{2+}_{(aq)} + 2NO_{2(g)} + 2H_2O_{(I)}$

  The below diagram sho 8(*ban1hw;a4e/bg:rrpn d0 w w /zjwcws an electrolytic cell. At which electrode will bromine form, and w*:whw e(w 0bz1n w;b4p/n d8rgr/ja achat is the process taking place there?

  The diagram below shows a Daniel cell. Zinc is more reactive than copper. Whe,tl:+nm 0ht lzy(w3g1nr f,ppn the spontaneous reaction occurs, which statement about the Daniel cell is correcp,n(m,t gp+1:lr0twlz fy n3ht?

  The equation for the overall reaction in a voltaisrz435v; kd-tqd,1kf 5uptp fc 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 q s;g6o,uyn,eq4kwu 2following sulfur-containing o ,;4ny,su 2gq 6ukeqwspecies?
$SO_3^{2-}, H_2SO_4, S_8, S_2O_3^{2-}$

  Alkali metals react with water to form jhgkqx)hh( u7 /5le(bmetal 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 whev.pp 0bh2ckn1zkjs vd8h/*9 yn nitrate changes to nitrite ?

Sodium metal may be obtained commercially from the electrolysis +3s*bdq nez-9i v 7 ujyb8vw6gof molten sodium chloride in a Downs cedgb*wzv3bjquv 6ie7sy 9- n8+ll. This cell operates as an 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 cox f+klxd1l;z 8ntainer 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 redox y u d)/fjt6weas1e,.zreaction:
$Cr_2O_7^{2-}(aq) + 14H^+(aq) + 6Ag(s) \rightarrow 2Cr^{3+}(aq) + 7H_2O(l) + 6Ag^+(aq)$
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 )dbyg l 0uf54rgalvanic 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 type and write its complet;5 mhm. uf8ukne balanced chemical equation using the structural formulas of reactants m58m;kh.nfuu 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 perc gi8s)ivyy 6wqac/-1) d(q pjyentage of copper present in a sample of copper (I) oxide. The sample is first dissolved in acidic sol( a/dis icp) yq) wj81yqv6-ygution 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 followiup p,yw(:+i ru/t y 4ulvfx/y-ng reactions involving metals and their aqueous nitrate solutionsv puu4 :yl upy,t-/+(/ fywixr:

	$XNO_3$	$Y(NO_3)_2$	$Z(NO_3)_2$
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 reale27sh/4p 0 1g weiedzctions:
$Fe(s) + Cu^{2+}(aq) \rightarrow Fe^{2+}(aq) + Cu(s)$
$Fe(s) + 2Ag^+(aq) \rightarrow Fe^{2+}(aq) + 2Ag(s)$
$Zn(s) + Fe^{2+}(aq) \rightarrow Zn^{2+}(aq) + Fe(s)$
$Cu(s) + 2Ag^+(aq) \rightarrow Cu^{2+}(aq) + 2Ag(s)$

  The equation below shows the reaction bgwtplct *p l q+e)(n s0vq08 :e1gm(eu+ *jptuetween concentrated sulfuric acid and potassium iodide. ) sp8w tq lmegpn0: 1*c0upvetq((*+jetu gl+
$8KI(s) + 5H_2SO_4(aq) \rightarrow 4K_2SO_4(aq) + 4l2(g) + H_2S(g) + 4H_2O(l)$
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 followin+,d(j/ix8e uutmcuo*g equations:
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