IBSL Chemistry Topic 5 Energetics Multiple Choice Questions
- 1.Which statement about this reaction is correct?
- A.
26.6 KJ of energy are released for every mole of Fe reacted
- B.
26.6 KJ of energy are absorbed for every mole of Fe reacted
- C.
53.2 KJ of energy are released for every mole of Fe reacted
- D.
13.3 KJ of energy are absorbed for every mole of Fe reacted
- 2.When solutions of HCl and NaOH are mixed the temperature increases. The reaction:
- A.
Is endothermic with a positive enthalpy energy
- B.
Is endothermic with a negative enthalpy energy
- C.
Is exothermic with a positive enthalpy energy
- D.
Is exothermic with a negative enthalpy energy
- 3.What can be deduced about the relative stability of the reactants and products and the sign of from the enthalpy level diagram above?
- A.
Products are more stable and sign of difference of enthalpy energy is negative
- B.
Products are more stable and sign of difference of enthalpy energy is positive
- C.
Reactants are more stable and sign of difference of enthalpy energy is negative
- D.
Reactants are more stable and sign of difference of enthalpy energy is positive
- 4.For the reaction: IF
- A.
The enthalpy difference for the third reaction must be negative
- B.
The enthalpy difference for the third reaction must be positive and smaller than 52.3 KJ
- C.
The enthalpy difference for the third reaction must be negative and larger than 52.3 KJ
- D.
No conclusion can be made without the value of H and H2(g)
- 5.The enthalpy changes for two different hydrogenation reactions of Which expression represents the enthalpy change for the reaction below?
- A.
DeltaH3 = deltaH1 + deltaH2
- B.
DeltaH3 = deltaH1 - deltaH2
- C.
DeltaH3 = deltaH2 - deltaH1
- D.
DeltaH3 = - deltaH1 - deltaH2
- 6.Use the bond energies for H-H (346kJ.mol-1) Br-Br (193 Kj mol-1) and H-Br (366 KJ mol-1) to calculate (in KJ mol-1) for the reaction:
- A.
263
- B.
103
- C.
-103
- D.
-263
- 7.The average bond enthalpy for the C-H bond is 412 KJ mol-1. Which process has an enthalpy change closest to this value?
- A.
CH4 (g) -> C(s) + 2 H2(g)
- B.
CH4 (g) -> C(g) + 2 H2(g)
- C.
CH4 (g) -> C(s) + 4 H (g)
- D.
CH4 (g) -> CH3(s) + H(g)
- 8.What energy changes occur when chemical bonds are formed and broken?
- A.
Energy is absorbed when bonds are formed and when they are broken
- B.
Energy is released when bonds are formed and when they are broken
- C.
Energy is absorbed when bonds are formed and released when they are broken
- D.
Energy is released when bonds are formed and absorbed when they are broken
- 9.The temperature of a 2.0g sample of aluminium increases from 25 to 30 degrees Celsius. How many joules of heat energy were added? Specific Heat Capacity of Al= 0.90 J.g-1. K-1
- A.
0.36
- B.
2.3
- C.
9.0
- D.
11
- 10.Using the eqautions below:
- A.
+910
- B.
+130
- C.
-130
- D.
-910
- 11.Question No Image
- A.
-570
- B.
-790
- C.
-860
- D.
-1080
- 12.The average bond enthalpies for O-O and for O=O are 146 and 496 KJ.mol-1 repectively. What is the enthalpy change, in KJ, for the reaction below? H-O-O-H (g) --> H-O-H (g) + 1/2 O=O (g)
- A.
-102
- B.
+102
- C.
+350
- D.
+394
- 13.The enthalpy changes for two different hydrogenation reactions of C2H2 are; C2H2 + H2 ->C2H4 DH1 C2H2 +2H2 -> C2H6 DH2 Which expression represents the enthalpy change for the reaction below? C2H4 + H2 -> C2H6 DH=?
- A.
DH1+ DH2
- B.
DH1 - DH2
- C.
DH2 - DH1
- D.
-DH1- DH2
- 14.The bond enthalpies of H2, Br2 and HBr are 436, 192, and 366 kJ mol-1 respectively. Use these values to calculate ∆H in kJ for the reaction; H2 (g) + Br2 (g) -> 2HBr(g)
- A.
+262
- B.
–104
- C.
–208
- D.
–262
- 15.N2 (g) + O2 (g) à 2NO(g) DH =180.4 kJ N2 (g) + 202 (g) -> 2NO2 (g) DH = 66.4 kJ Use the enthalpy values above to calculate DH for the reaction: NO(g) + ½ O2 (g) -> NO2 (g)
- A.
-57 kJ
- B.
-114 kJ
- C.
57 kJ
- D.
114 kJ
- 16.Which statement about this reaction is correct? 2Fe(s) + 3CO2 (g) -> Fe2O3(s) + 3CO(g) DH = +26.6 kJ
- A.
26.6 kJ of energy are released for every mole of Fe reacted
- B.
26.6 kJ of energy are absorbed for every mole of Fe reacted
- C.
53.2 kJ of energy are released for every mole of Fe reacted
- D.
13.3 kJ of energy are absorbed for every mole of Fe reacted
- 17.Which statement about exothermic reactions is not correct?
- A.
They release energy
- B.
The products have a greater enthalpy than the reactants
- C.
The enthalpy change (∆H) is negative
- D.
The products are more stable than the reactants
- 18.In an experiment to measure the heat change when a small amount of sodium hydroxide is dissolved in water, x g of sodium hydroxide was dissolved in y g of water, giving a temperature rise of z OC. The specific heat capacity of water is c Jg−1 K-1. Which expression should be used to calculate the heat change (in J )?
- A.
Cxyz
- B.
Cyz
- C.
Cxz
- D.
Cxy
- 19.Some average bond enthalpies (in kJ mol−1) are as follows: H–H =436 , Cl–Cl =242 , H–Cl =431 What is the enthalpy change (in kJ) for the decomposition of hydrogen chloride? 2HCl →H2 +Cl2
- A.
−184
- B.
+184
- C.
+247
- D.
−247
- 20.When solid ammonium nitrate dissolves in water, the temperature decreases. Which statement about the dissolving of ammonium nitrate in water is correct?
- A.
It is endothermic with ∆H greater than zero.
- B.
It is endothermic with ∆H less than zero.
- C.
It is exothermic with ∆H less than zero.
- D.
It is exothermic with ∆H greater than zero.
- 21.When 0.01 mol of solid NaOH is added to 100 cm3 of 1.0 mol dm−3 HCl, the temperature increases by ∆T1. What will be the temperature change, ∆T2, for a second experiment in which the amount of NaOH and the volume of 1.0 mol dm−3 HCl are each doubled?
- A.
∆T2=∆T1
- B.
∆T2=1/2 ∆T1
- C.
∆T2=2∆T1
- D.
∆T2=4∆T1
- 22.O2(g) →2O(g) ∆H= 498 kJ 3O2 (g) →2O 3 (g) ∆H= 284 kJ Using the information above, what is ∆H for the following equation in kJ?
- A.
605
- B.
463
- C.
356
- D.
214
- 23.Which statement about endothermic reactions is not correct?
- A.
They have positive ∆H values.
- B.
Products have a higher enthalpy than the reactants.
- C.
They release energy.
- D.
Products are less thermally stable than the reactants.
- 24.The enthalpy changes for two reactions involving hydrogen are as follows: C(s) +2H2 (g) →CH4(g) ∆H = − 75 kJ H2(g) →2H(g) ∆H = + 436 kJ What is the enthalpy change (in kJ) for the reaction CH4 (g) →C(s) +4H(g) A. −947 B. +361 C. +511 D. +947
- A.
+947
- B.
+511
- C.
+361
- D.
−947
- 25.Which reaction has an enthalpy change equal to four times the bond enthalpy of the C−H bond?
- A.
CH4 (g) → C(s) + 2H2 (g)
- B.
CH4 (g) → C(s) + 4H(g)
- C.
CH4(g) → C(g) + 4H(g)
- D.
CH4 (g) → C(g) + 2H2 (g)
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