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- 1. Multiple ChoiceEnergy in exothermic reactions arereleasedabsorbed
- 2. Multiple ChoiceEndothermic reactions feelwarmcold
- 3. Multiple ChoiceWhich statement is true regarding endothermic reactions?a) Temperature change is positive and enthalpy change is positiveb) Temperature change is positive and enthalpy change is negativec) Temperature change is negative and enthalpy change is positived) Temperature change is negative and enthalpy change is negative
- 4. Multiple Choice
Which of the following shows the enthalpy of formation of sodium iodide
Na(s) + 1/2 I2(s) --> NaI(s)
Na(s) + 1/2 I2(g) --> NaI(s)
Na(s) + I(g) --> NaI (s)
Na+(g) + I-(g) --> NaI (s)
- 5. Multiple Choice
10. Which label on the diagram accurately identifies the Activation energy for an endothermic reaction? a) A b) B c) C d) DCDEF - 6. Multiple Choice
How do you calculate Enthalpy of a reaction?
ΔH = ΔHproducts - ΔHreactants
ΔT = q / mC
ΔG = ΔH -TΔS
E = mc2
- 7. Multiple ChoiceRefer to the following question:
2N2 + 3H2 --> 2NH3 + 46 kJ
How much energy would be produced if only 1 mol of nitrogen was reacted?92 kJ0.143 kJ23 kJ15 kJ - 8. Multiple Choice
Calculate the enthalpy of reaction (ΔH).
4CO2 (g) + 6H2O (g) → 2C2H6 (g) + 7O2 (g)
ΔHfo [CO2(g)] = -393.5 kJ
ΔHfo [H2O(g)] = -241.8 kJ
ΔHfo [C2H6(g)] = -84.7 kJ
550.647 KJ/mol
2855.584 KJ/mol
-550.647 KJ/mol
-2855.584 KJ/mol
- 9. Multiple ChoiceWhen ammonium nitrate dissolves in water, the solution gets cold. Which is true?Reaction is ENDOTHERMIC with positive ΔHReaction is ENDOTHERMIC with -ΔHReaction is EXOTHERMIC with a -ΔHReaction is EXOTHERMIC with +ΔH
- 10. Multiple ChoiceSpecific heat capacity isheat energy needed to raise temp by 1Cheat energy needed to raise temp of 1g of substance by 1Cheat energy absorb to raise 1g of substance to higher tempheat energy need to raise temp for 1g of substance
- 11. Multiple Choice
"Heat change when 1 mole of gaseous atom is formed from its element at standard states" is the definition for _______.
standard enthalpy of formation
standard enthalpy ofhydration
electron affinity
standard enthalpy of atomisation
- 12. Multiple Choice
What is standard enthalpy of formation, ΔHfo?
Heat change when 1 mole of gaseous ions is hydrated in water at 25oC and 1 atm
Heat change when 1 mole of compound is formed from its elements in their standard states at 25oC and 1 atm
Heat change when 1 mole of gaseous atom is formed from its elements at 25oC and 1 atm
Heat change when 1 mole of electrons is removed from 1 mole of gaseous atoms at ground state at 25oC and 1 atm
- 13. Multiple Choice
How to find the absolute enthalpy of a substance?
using formula
predict the answer
(final enthalpy) - (initial enthalpy)
none of the above
- 14. Multiple Choice
Name the type of enthalpy for the following reaction:
Na+ (g) --> Na+ (aq) ΔH = -364 kJmol-1
Standard enthalpy of neutralisation, ΔHneuto
Standard enthalpy of solution, ΔHsolno
Standard enthalpy of hydration, ΔHhydo
lattice energy, ΔHlatticeo
- 15. Multiple Choice
Enthalpy change represented by the equation
MgSO4 (s) ---> Mg2+ (aq) + SO4 2- (aq)
is known as_____________.
ionization energy of magnesium and sulphate
lattice crystal energy of magnesium sulphate
enthalpy of solution of magnesium sulphate
enthalpy of hydration of magnesium sulphate
- 16. Multiple Choice
Define standard enthalpy of combustion.
Heat released when one mole of substance is burnt completely in excess oxygen.
Heat absorbed when one mole of substance is burnt completely in excess oxygen under standard state.
Heat released when one mole of substance is burnt completely in excess oxygen under standard state.
Heat change when one mole of substance is burnt partially in excess oxygen under standard state.
- 17. Multiple Choice
Which of the following has a ΔHfo value of 0?
Br2(g)
N(g)
CO(g)
Ne(g)
- 18. Multiple Choice
What is the type of standard enthalpy of this reaction?
Na(s) ---> Na(g) ΔH = +109 kJmol-1
standard enthalpy of formation
standard enthalpy of combustion
standard enthalpy of atomisation
standard enthalpy of hydration
- 19. Multiple Choice
Which of the equation below refers to the standard enthalpy of formation, ΔHfo?
Na(g) ---> Na+(g) + e- ΔH = -364 kJmol-1
C2H5OH(l) + 3O2(g) ---> 2CO2(g) + 3H2O (l) ΔH = - 1286 kJmol-1
2C(s) + 2H2(g) ---> C2H4 (g) ΔH = - 52.3 kJmol-1
Na+(g) ---> Na+(aq) ΔH = - 364 kJmol-1
- 20. Multiple Choice
When 1.0 mole of ZnO(s) decomposes,
ZnO(s) ---> Zn(s) + 1/2 O2(g) , enthalpy change is +348 kJ/mol.
What does this tell you about the formation of ZnO (s)?
the formation of ZnO (s) is endothermic
the formation of ZnO (s) is exothermic
the formation of ZnO (s) does not require energy
the formation of ZnO (s) absorbs heat.
- 21. Multiple Choice
The enthalpy of formation of sodium acetate CH3COONa is -14.4 kJ mol-1.
Which of the following is the correct thermochemical equation?
CH3COO-(aq) + Na+ (aq) --> CH3COONa (s) ΔH = -14.4 kJ mol-1
C(s) + H2 (g) + O (g)+ Na (s) --> CH3COONa (s) ΔH = -14.4 kJ mol-1
C(s) + 3/2 H2 (g) + O2 (g)+ Na (s) --> CH3COONa (s) ΔH = -14.4 kJ mol-1
2C(s) + 3/2 H2 (g) + O2 (g)+ Na (s) --> CH3COONa (s) ΔH = -14.4 kJ mol-1
- 22. Multiple ChoiceWhat type of reaction is shown in the reaction pathway?endothermic reactionexothermic reaction
- Answer choicesTagsAnswer choicesTags