Which of the following2 v crdt;)ajapus z/:9 statements is false?

  Choose the correct equation for thenh 7z3:uoa(i-ubju /d diagram below:

  Which of the following is correct in an endothermibot4iv + n)uc-c reaction?

  Which shows the oxygen-to-oxygen bonds in order of increasing averagjv6a-fv /n7,jarp t. ap1u * jd+f*dade bond enthalpy rju.d7*p1 j n,ap6*jdaa/fa- td +vvf?

  Which expression gives the enthalpy changl;9h- g+njc sie, ΔH, for the production of hydrated copper (II) sulfate f i9jc h-;n+glsrom its anhydrous salt:

  Which statement about Born-Haber cycles is sbm8 :; 3v,,wuky9 pozfvw :dxnot correct?

  What is the enthalpy9 f ndv n nt7ti.n4nh1hvm)q)9 ΔH$_1$ in kJmol$^{-1}$?

  Which enthalpy change cannot be calculated directly fro:a *3amf fi *6hxnwn2i69vueom average bond enthalpy data?x6f6w i*f n3hi9:oun e*vaam 2

  Which statements about average bond entha2.i m* 4:m gbe8eo+;c brvzjhw; eje(ilpies are correct?
I.Average bond enthalpies are endothermic
II.Average bond enthalpies depend on the strength of the covalent bonds
III.Average bond enthalpies are unique to the covalent bonds in a specific compound

  The following diagram shows the enthalpy of the reactants2xx8:ov r1v kk and products of a reaction involving gaseous covalent compound2 v 1kov8r:kxxs. Which statement is correct?

  Given the enthalpy changes forte6q0-m2w z-v el1xii the reactions below.
$\frac{1}{2}$$N_2$(g)+$O_2$(g)→$NO_2$(g); ΔH=+33.9kJ
$NO$(g)+$\frac{1}{2}$$O_2$(g)→$NO_2$(g); ΔH=-56.5kJ
What will be the enthalpy change for:
$\frac{1}{2}$$N_2$(g)+$\frac{1}{2}$$O_2$(g)→$NO$(g)?

  Hydrocarbons are common lvih7). )qxchly used as fuels.
1.1Define average bond enthalpy.
1.2Write a balanced chemical equation for the complete combustion of propene ($CH_3CHCH_2)$

2.Using section 11 (Section 12- 2025 Syllabus) of the data booklet, calculate the enthalpy of combustion for propene.
ΣΔH$_{BE}^θ$(bonds broken)=  kJ mol$^{-1}$ ;ΣΔH$_{BE}^θ$(bonds formed)=  kJ mol$^{-1}$;ΔH=-  kJ mol$^{-1}$
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 for the 2025 syllabus.

  Given the following informao db+ 7u+x,8ns9ej jnwc)5pmv tion:
C(s)+$O_2$(g)→$CO_2$(g); ΔH= -393.5kJ mol$^{-1}$
CO(g)+$\frac{1}{2}$$O_2$(g)→$CO_2$(g);ΔH= -283.0kJ mol$^{-1}$
The standard enthalpy of formation of carbon monoxide (CO) is:

  Which expression represents the enthalpy change 3.0n:5s jjh zcr1r5myacj 2vg for $CO$(g)+$H_2O$→$CO_2$(g)+$H_2$(g)?

  Which statement about ozone is correctxii2km1m2 fah*e z7 j2?

  Ethene reacts with hydrogen b sjfqd. :)w)avi0e ea3romide at 298 K and 100 k Pa pressure to produce bromoethane. All three compounds are gases under these conditions.The enthalpy change of this reaction, d 0q3a:)e.vejw )af isΔH$_r$, an be estimated from the enthalpies of formation (Method 1) or average bond enthalpies (Method 2) of the reactants and products. The enthalpy cycles used in these calculations are shown.

?
Which method gives the least accurate estimate of ΔH$_r$

  Using the table below, choca/on:d f c4ai;* hqx,ose the correct expression that represents the enthalpy cxon /4,ch:cda q af*i;hange for the following hydrogenation reaction:
$C_2H_4$(g)+$H_2$(g)→$C_2H_6$(g)

Substance is $C_2H_4$(g) ; ΔH (Enthalpy of Formation) kJ mol$^{-1}$ is x
Substance is $C_2H_6$(g) ; ΔH (Enthalpy of Formation) kJ mol$^{-1}$ is y

  1.Define standard enthalpy of formatio0k5e3w 8 9xx+hjomb lxhv)p( fn.
2.Draw a Hess diagram for the following reaction:
2$CO$(g)+$O_2$→$CO_2$(g)
Make sure to label all enthalpies of formation.
3.Refer to section 12 (Section 13- 2025 Syllabus) of the data booklet to calculate the enthalpy of reaction, ∆H$^ᶱ_r$, for:
2$CO$(g)+$O_2$→$CO_2$(g)
∆H$^ᶱ_r$=-  kJ mol$^{-1}$
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 for the 2025 syllabus.

  What is the enthalpy changfv 8ru0r6l 5j avfv0l:e for the combustion of methane:
$CH_4$(g)+2$O_2$(g)→$CO_2$(g)+2$H_2O$(g) in kJmol$^{-1}$?

  Ethanol can be produced through the f6* pe vytz,4bcermentation of glucose:
$C_6H_12O_6$(aq)→2$C_2H_5OH$(l)+2$CO_2$
1.1.Predict whether the entropy change for this reaction is positive or negative. Explain your reasoning.
1.2.The absolute entropy for glucose is +209.2JK$^{-1}$mol$^{-1}$ . Using section 12 (Section 13- 2025 Syllabus) of the data booklet, calculate the entropy change for this reaction.
ΔS$_{reaction}$=+  K$^{-1}$mol$^{-1}$.
2.The enthalpy of formation of glucose is -1273.3kJmol$^{-1}$ .Using section 12 (Section 13- 2025 Syllabus) of the data booklet, calculate the enthalpy change for this reaction.
ΔH$_{reaction}$=-  kJ mol$^{-1}$
3.Using your answers to (a)(ii) and (b), calculate the Gibbs free energy change at 298K.
ΔG=-  kJ mol$^{-1}$
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.

  Refer to the Born-Haberz(lg0 +pe nip. cycle for potassium chloride below:

What is the correct name for the enthalpy changes labeled x, y, and z?

State Hess’s law.
Suggest why it may be useful to use Hess’s law to determine the heat of formation.
Calculate a value for ΔH$_f^θ$ [$CH_3OH(l)$] using the enthalpies of combustion data from section 13 (Section 14- 2025 Syllabus) of the Data Booklet.
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 for the 2025 syllabus.

  When a sample of solidc(bj)1 1eot ik calcium carbonate is placed in hydrochloric acid, the following reaction takes pla(coj tk)ie11b ce.
$CaCO_3$(s)+2HCl(aq)→$CaCl_2$(aq)+$H_2O$(l)+$CO_2$
The temperature and mass of the solution are both monitored, as shown.


1.The standard enthalpies of formation of hydrochloric acid and the products of its reaction with calcium carbonate are shown.


.1.Define the term standard enthalpy of formation.
.2.Calculate the standard enthalpy of formation of calcium carbonate, in kJmol$^{-1}$.
2.A reaction profile shows how the enthalpies of the molecules in a reactant change as the reaction progresses.
Part of the reaction profile for the reaction of calcium carbonate and hydrochloric acid is shown.


Complete the reaction profile by showing how the enthalpy changes between the reactants and products and labelling the value of Δ$H_r^Θ$.

3.The sample of calcium carbonate is added to 100 cm$^3$ of dilute hydrochloric acid. During the reaction, the mass of the conical flask and its contents decreases by 6.28g due to the loss of carbon dioxide gas. The molar mass of carbon dioxide is 44.0g mol$^{-1}$.

.1.Calculate, to 1 decimal place, the maximum possible change in the temperature of the solution, using sections 1 and 2 of the data booklet. You should assume that the solution has the same density and specific heat capacity as water and does not change in mass during the reaction.ΔT=(+)  ( $^{\circ}C$ ).

.2.The measured change in temperature is much less than the maximum possible value. State why the experimental and theoretical results are different, assuming that the value of Δ$H_r^Θ$, is accurate.
.3.Suggest why the measured mass loss during the reaction is likely to be less than the mass of carbon dioxide produced.

  Cracking is a process by which gaseous alkan,uqw-nvap;eo:7.b w0em: k lb- l x+dhes are converted to smaller-chain alkanes and alkenes.xnb+ul0q . -7-,;bohavk: we:lpwemd One possible reaction in the cracking of butane is shown.


What is the enthalpy change of the cracking reaction?

  Consider the formation 8z knntm7m61 ; qa+kaiof water:
$H_2$(g)+$\frac{1}{2}O_2$(g)→$H_2O$(l)
1.Using section 11 (Section 12- 2025 Syllabus) of the data booklet, calculate the enthalpy change for this reaction.
ΔH =-  kJ mol$^{-1}$
2.1.Compare the theoretical value of enthalpy of formation of water found in section 12 (Section 13- 2025 Syllabus) of the data booklet to your answer in part (a). Suggest two reasons why they differ.
2.2.State the enthalpy change required to make your answer in part (a) more accurate.
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 for the 2025 syllabus.

  In the presence of a catalyst, aqueous hydrogen peroxide decompt * k3,xwp.magoses into water and oxygen. The equation for a .t3*km,pwxg this reaction and the enthalpy change
ΔH$_{dec}^{θ}$ is related to three other enthalpy changes,ΔH$_{A}^{θ}$,ΔH$_{B}^{θ}$ and ΔH$_{C}^{θ}$.

.1.State the name given to the enthalpy change labelled ΔH$_{A}^{θ}$.The name is    (of aqueous hydrogen peroxide)

.2.Calculate ΔH$_{A}^{θ}$ in kJ mol$^{-1}$ using the information in the enthalpy cycle and section 12 (Section 13- 2025 Syllabus) of the data booklet.ΔH$_{A}^{θ}$=  kJ mol$^{-1}$.

2.A solid catalyst was added to 100 cm$^{-1}$ of an aqueous hydrogen peroxide solution and the temperature was monitored using a thermometer. The resulting temperature-time graph is shown.



The maximum theoretical temperature change during the reaction, ΔT, is determined by the molar concentration of hydrogen peroxide,[$H_2O_2$]
.1.State why ΔT is determined by extrapolating the trend of the temperature profile between 65 and 120 s.
.2.Using the value of ΔH$_{dec}^{θ}$ the information in the temperature-time graph and sections 1 and 2 of the data booklet, calculate the initial concentration of the hydrogen peroxide solution in mold\m$^{-3}$.
Assume that the specific heat capacity of the solution is 4.18J g$^{-1}$K$^{-1}$. [$H_2O_2$] =  mold\m$^{-3}$.
3.The decomposition of gaseous hydrogen peroxide into water vapour and oxygen is an important atmospheric reaction.
.1.Calculate the enthalpy change of this reaction, using the bond enthalpy values in section 11 (Section 12- 2025 Syllabus) of the data booklet.
Enthalpy change=-  (kJ mol$^{-1}$)
.2.Suggest one reason why the enthalpy change calculated in (i) differs from the enthalpy change for the decomposition of aqueous hydrogen peroxide.

  1.Define standard enthalpy of combusc f*+s*ic-5 9h slgiwxtion.
2.Outline how Hess’s law differs or concurs with the law of conservation of energy.
3.Using the equation provided below, draw a Hess’s law diagram using enthalpy of combustion equations, and calculate the enthalpy change for the hydrogenation of ethene using section 13 (Section 14- 2025 Syllabus) of the data booklet.
$C_2H_4$(g)+$H_2$→$C_2H_6$
ΔH$_r$=-  kJ mol$^{-1}$
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 for the 2025 syllabus.

  Consider the following reactionv.hr any4 q8zu2i:6sd :

$C_2H_4$(g)+$H_2$(g)→$C_2H_6$(g)

ΔH −136kJ mol$^{-1}$
ΔS −121JK$^{-1}$mol$^{-1}$
ΔG at 298K −99.9kJ mol$^{-1}$

1.1Explain why the enthalpy of formation of $H_2$ is 0kJmol$^{-1}$.
1.2Explain why the entropy change for this reaction is negative.
2.Explain how a reaction can be spontaneous with a negative entropy change.
3.Calculate the temperature at which this reaction is no longer spontaneous.
T=  K

  The enthalpies of combus zgf )um*xf+l:tion of hydrogen and carbon are given in the data booklet. The enthalpy of formation:*ugxml)fz f+ of ethene,$C_2H_4$,from its elements is ΔH$_f^θ$=+52.0kJ mol$^{-1}$.
1.Write the thermochemical equation for the formation of ethene.
2.Calculate the enthalpy of formation of ethene, using enthalpies of combustion from section 13 (Section 14- 2025 Syllabus) of the Data Booklet. Then compare to the given value above, and comment on the difference, if any.
ΔH$_r$=+  kJ mol$^{-1}$.
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 for the 2025 syllabus.

  Carbon monoxide is produced when there is insufficient oxygen in combustion r)i 0uf q:gmtnsj; qm2o+3uemgu)1 apo1(y,ineactions. It reacts with oxyuoy1n +j3,s g)q;q2iugf:na0 up 1mt i)o m(megen to produce carbon dioxide according to the following equation: $CO$(g)+$\frac{1}{2}$$O_2$(g)→$CO_2$(g).

1.Define enthalpy change of combustion.

2.Using sections 11 and 13 (Sections 12 and 14- 2025 Syllabus) of the data booklet, calculate the average bond enthalpy for C≡O.

ΔH $_{BE}^{θ}$ (C≡O)=  kJ mol $^{-1}$

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 for the 2025 syllabus.

  Sulfur dioxide ($SO_2$) reacts with oxygen and sulfuric acid($H_2SO_4$) to produce oleum($H_2S_2O_7$) in two reaction steps. The enthalpy cycle for this process is shown.

This process is used to produce a dilute solution of oleum in 5000g sulfuric acid from 0.80 mol sulfur dioxide. During the reaction, the temperature of the sulfuric acid increased by 22.8$^{\circ}C$.
What are the enthalpy changes of the second step,ΔH$_2$, and the overall process, ΔH$_total$, assuming no heat is lost during the reaction?
·Specific heat capacity of $H_2SO_4$,c=1.60Jg $^{-1}$K$^{-1}$;
·q=mcΔT.

  Liquid dinitrogen tetroxidfp2-5+ raj v*(q wp+kxelwq4 zik0v4ne ($N_2O_4$) is converted to gaseous nitrogen dioxide when heated, as shown in the diagram. No other molecules react or form during this reaction.


The standard enthalpy change of the reaction,ΔH$_r^θ$, is +85.8kJmol$^{-1}$.The standard enthalpy of formation of gaseous $NO_2$ , ΔH$_r^θ$($NO_2$), is +33.1kJmol$^{-1}$.
What is the standard enthalpy of formation of liquid $N_2O_4$,ΔH$_r^θ$($N_2O_4$)?

  Hydrazine ($N_2H_4$) is a commonly used rocket fuel.
The rocket is propelled by the decomposition of liquid hydrazine into nitrogen and hydrogen gases. The equation and enthalpy change of this decomposition reaction are shown.



1.Hydrazine may also decompose via the following reactions:
Reaction 2: 3$N_2H_4$→4$NH_3$+$N_2$
Reaction 3: $N_2H_4$+4$NH_3$→3$N_2$+8$H_2$
The enthalpy changes of reactions 2 and 3 are ΔH$_2$ and ΔH$_3$, respectively.
Explain why it is possible to calculate ΔH$_1$ from ΔH$_2$ and ΔH$_3$
2.Using section 12 of the data booklet, calculate an alternative value for ΔH$_1$ in kJ mol${-1}$.
ΔH$_1$=-  (kJ mol${-1}$)
3.Suggest two reasons why the value calculated in (b) differs from the measured value of ΔH$_1$.

  The standard enthalpy of formatit9rw,ey v:bwxt dg)ai*e(8 1ion of gaseous nitric oxide,ΔH$_f^θ$(NO(g)),is +90.3kJmol$^{-1}$.
1.Write a reaction equation, including state symbols, corresponding to the standard enthalpy of formation of gaseous nitric oxide.
2.Calculate the bond enthalpy of nitric oxide, using the value of ΔH$_f^θ$(NO(g)) above and section 11 (Section 12- 2025 Syllabus) of the data booklet.
E(N≡O)=  (kJ mol$^{-1}$)
3.In the Ostwald process, nitric oxide (NO) is reacted with oxygen and then water to produce aqueous nitric acid($HCO_3$).The overall equation and enthalpy change of this reaction are given below.
4NO(g)+3$O_2$(g)+2$H_2O$(l)→4$HNO_3$(aq)
ΔH$_1$=-576.4kJ mol$^{-1}$
Calculate the enthalpy of formation of aqueous nitric acid, ΔH$_f^θ$($HNO_3$(aq)),using the values of ΔH$_f^θ$(NO(g))=+90.3kJ mol$^{-1}$,and ΔH$_1$ and section 12 (Section 13- 2025 Syllabus) of the data booklet.

ΔH$_f^θ$($HNO_3$(aq))=  (kJ mol$^{-1}$)
4.The nitric oxide used in the Ostwald process is formed by reacting gaseous ammonia ($NH_3$) with oxygen. The equation and enthalpy change of this reaction are given below.
4$NH_3$(g)+5$O_2$(g)→4$NO$(g)+6$H_2O$(g)
ΔH$_2$=-906.0kJ mol$^{-1}$
The yield of the Ostwald process may be lower than expected if some of the nitric oxide product reacts with the remaining ammonia. The equation for this side reaction is shown.
4$NH_3$(g)+6$NO$(g)→5$N_2$(g)+6$H_2O$(g)
4.1Calculate the enthalpy change for the side reaction, Δ$H_{side}$,using the values of ΔH$_f^θ$(NO(g)) and ΔH$_2$.
Δ$H_{side}$=-  (kJ mol$^{-1}$)
2.Suggest how the value of ΔH$_2$ would differ if water were produced in the liquid phase.
The value of ΔH$_2$ would be  ----待选择----largerless  negative