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WorksheetsS1-Q4-U4 - L1 all
Total questions: 15
Worksheet time: 1hrs 16mins
Given the following data: ΔH○f[FeO(s)] = –270kJmol–1
ΔH○f [Fe2O3(s)] = –820 kJ mol–1
Select the expression which gives the enthalpy change, in kJ mol–1, for the reaction:
2FeO(s) + 1⁄2O2(g) → Fe2O3(s)
–140
–1090
–280
+280
–550
What is the enthalpy change under standard conditions for the following reaction?
3FeO(s) + 2Al (s) -> 3Fe(s) + Al2O3(s)
Which statement about this information is correct?
than the total energy of the bonds
formed in the product
Ethene and iodine react to form 1,2-diiodoethane. The equation for this reaction is shown, the total energy change per mole of ethene is (-24 KJ/mol) if the bond energies are [C-C is 346 ; C=C is 602 ; C-H is 411 ; I-I is 148] , calculate the bond energy of C-I ??
2031 KJ
387 KJ
214 KJ
598.5 KJ
Which of the following hydrogen halides has the smallest bond enthalpy?
HF
HCl
HBr
HI
Chloromethane is produced by the reaction of methane CH4 with chlorine gas in the presence of UV light. The equation for this reaction is shown.
calculate the molar heat enthalpy for this reaction ?
[C-H = 411 ; H-Cl=428 ; Cl-Cl=240 ; C-Cl=327]
-104 KJ
+104 KJ
+327 KJ
-250 KJ
The process of dissolution can be considered to involve three steps. Which of the following is not one of these steps?
The separation of solvent–solute interactions
The separation of solvent–solvent intermolecular attractions
The formation of solute–solvent interactions
The separation of solute–solute attractions
What is the enthalpy change of dilution, Δ𝐻dil?
71.2 KJ
-13.2 KJ
-71.2 KJ
+ 13.2 KJ
what do X and Y represent respectively?
ΔH melting & Δ H evaporation
ΔH Fusion & Δ H evaporation
ΔH condensation & Δ H evaporation
ΔH Fusion & Δ H solution
What standard enthalpy change can be defined as the enthalpy change when one mole of a substance transforms from a liquid state to a solid state under standard conditions?
Standard enthalpy of fusion
Standard enthalpy of vaporization
Standard enthalpy of sublimation
Standard enthalpy of solidification
Standard enthalpy of condensation
Which of the following values is equivalent to Δ𝐻3?
−Δ𝐻1+Δ𝐻2+Δ𝐻4
Δ𝐻1 - Δ𝐻2 - Δ𝐻4
− Δ𝐻1- Δ𝐻2 - Δ𝐻4
+ Δ𝐻1+Δ𝐻2+Δ𝐻4
Considering the diagram, which of the following equations would Hess’s law predict to be true?
Δ𝐻2=Δ𝐻3−Δ𝐻1
Δ𝐻1=Δ𝐻2+Δ𝐻3
Δ𝐻1=Δ𝐻2-Δ𝐻3
Δ𝐻2=Δ𝐻3+Δ𝐻1
The reaction represents ……. reaction
Exothermic
endothermic
Neither exothermic nor endothermic
A piece of copper of mass 400 g absorbed a quantity of heat of 9360 J & its temperature raised from 20˚C to 50˚C. What is the specific heat of copper?
0.78 J/gC
1.282 J/gC
7.8 J/gC
4.18 J/gC
Determine the final temperature when a 25 g piece of iron at 85˚C is placed into 75 g of water at 20˚C. (given that: specific heat of iron is 0.45 & water equals 4.184 j/g.˚C)
52.5 °C
22.25 °C
60.5 °C
45.25 °C
