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- 1. Multiple Choice
How do you calculate Enthalpy of a reaction?
ΔH = ΔHproducts - ΔHreactants
ΔT = q / mC
ΔG = ΔH -TΔS
E = mc2
- 2. Multiple Choice
Specific 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 - 3. Multiple Choice
"Heat change when 1 mole of gaseous atom is formed from its element at standard condition" is the definition for _______.
standard enthalpy of formation
standard enthalpy ofhydration
electron affinity
standard enthalpy of atomisation
- 4. 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 stable state at standard condition of 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
- 5. 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
- 6. 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
- 7. 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 conditionj
Heat released when one mole of substance is burnt completely in excess oxygen under standard condition.
Heat change when one mole of substance is burnt partially in excess oxygen under standard condition.
- 8. Multiple Choice
Which of the following has a ΔHfo value of 0?
Br2(g)
N(g)
CO(g)
Ne(g)
- 9. 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
- 10. 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
- 11. 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.
- 12. 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
- 13. Multiple ChoiceEndothermic reactions feelwarmcold
- 14. Multiple ChoiceDefine 'Enthalpy'a) Energy stored in the movement of molecules in a substanceb) The opposite of temperaturec) The temperature of a moleculed) Energy stored in the chemical bonds in a substance
- 15. Multiple ChoiceHeat is measured injoulesgramsdegrees celcius
- 16. Multiple ChoiceDescribe the energy change that takes place when bonds are broken.a) Energy is given outb) Energy is taken inc) Energy is taken in and then given outd) Energy is given out and then taken in
- 17. Multiple ChoiceWhich is an example of an endothermic physical reaction?a) Ice meltingb) Combustionc) Steam condensingd) Photosynthesis
- 18. Multiple ChoiceCalorimetry is a technique used tomeasure temperature changemeasure heat releasedmeasure heat absorbedmeasure the enthalpy change for a reaction
- 19. Multiple ChoiceWhich statement is FALSE for an exothermic reaction?Reactants higher in energy and less stableProduct lower in energy and more stableProducts have stronger bonds than reactantsReactants have stronger bonds than products
- 20. Multiple Choice
Diagram below shows
lattice energy
Standard enthalpy of precipitation
Standard enthalpy of formation
Standard enthalpy of hydration
- 21. Multiple Choice
Diagram below shows
Lattice energy
Standard enthalpy of solution
Standard enthalpy of formation
Standard enthalpy of hydration
- 22. Multiple ChoiceΔH value in an endothermic reaction is a positive number.TrueFalse
- 23. Multiple Choice
What does the circle mean in ΔH°?
Standard Conditions (T=298.15 K P=1 atm)
Standard Temperature and Pressure (T=273.15 K P=1 atm)
Degree K
Degree C
- 24. Multiple ChoiceThe SI unit of heat and energy is the __________.calorieheatjoulewatt
- 25. Multiple ChoiceWhat type of reaction is shown in the reaction pathway?endothermic reactionexothermic reaction
- 26. Multiple Choice
Match the definition below to the correct term.
The enthalpy change that takes place when one mole of a compound is formed from its elements in their standard states under standard conditions.
The enthalpy of neutralisation
The enthalpy of combustion
The enthalpy of formation
The enthalpy of reaction
- 27. Multiple Choice
Which of the following has a ΔHfo value of 0?
Br2(g)
N(g)
CO(g)
N2(g)
- 28. Multiple Choice
Define the term Exothermic by picking the correct statements
Products have less energy than the reactants
ΔH is negative
ΔH is positive
Energy is given out to the surroundings (temperature goes up).
products have more energy than the reactants
- 29. Multiple Choice
Define Endothermic by picking the correct statements
ΔH is positive
Energy is taken in from the surroundings (temperature goes down).
Energy is given out to the surroundings (temperature goes up).
· Products have less energy than the reactants
products have more energy than the reactants
- 30. 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
- 31. Fill in the Blank
Standard enthalpy change of formation, ΔfHΘ, is the enthalpy change that takes place when one mole of a compound is formed from its .................. under standard conditions (with all reactants and products in standard states).
- 32. Fill in the Blank
What value in kJ mol-1 is the standard enthalpy change of formation, ΔfHΘ, of any element?
- 33. Multiple Choice
The enthalpy of neutralisation is the enthalpy change
when one mole of the pure compound is formed from its elements under standard conditions
when 1 mole of pure substance is completely burned in excess oxygen, under the given temperature and pressure of the reaction
when 1 mole of H+ (aq) ions from acid reacts with 1 mole of OH- (aq) ions from an alkali to form 1 mole of water under the stated condition of the experiment
the magnitude of the enthalpy change of a chemical reaction depends only on the difference in the enthalpy content of the products and the reactants, and does not on how the reaction is completed
- 34. Multiple ChoiceFor which of these processes is the value of ΔH expected to be positive?
1. The temperature increases when calcium chloride dissolves in water.
2. Steam condenses to liquid water
3. Water boils
4. Dry ice sublimates4 only1 only3 and 4 only2 and 3 only - 35. Multiple Choice
What is the name of this enthapy change
Enthalpy of formation
Enthalpy of combustion
Enthalpy of reaction
Enthalpy of atomisation
- 36. Multiple Choice
Which of the following equations represents the enthalpy change of combustion?
2C4H10(g) +13O2(g) → 8CO2 (g) + 10H20(g)
C4H10(g) +13/2O2(g) → 4CO2 (g) + 5H20(g)
C4H10 + 9/2O2 = 4CO (s)+ 5H2O
C4H10 + 5/2O2 = 4C(s) + 5H2O(g)
- 37. Multiple ChoiceC+ O2 --> CO2 + 60kJ, what is the value for ΔH for the reaction?+60-60there is no way to know
- 38. Multiple Choice
What is the standard enthalpy change of formation?
2Fe (s) + 11/2O2(g) → Fe2O3(s)
4Fe (s) + 3O2 → 2 Fe2O3(s)
2H2(g) + O2 (g) → 2H2O (l)
- 39. Multiple Choice
For a skillet, used for cooking, do you want a high or low specific heat
High, so that it will need more energy to heat up
Low, so that it will change temperature quickly
- 40. Multiple ChoiceCalorimeters use insulating materials to:encourage affordable materials in science experiments in schools.preserve the heat of the environment outside the Styrofoam cup.prevent heat from escaping to the environment.keep the liquid inside the Styrofoam cup from overheating.
- 41. Multiple Choice
The amount of energy required to raise the temperature 1ºC for every gram is called____?
Thermal Energy
Specific Heat Capacity
Temperature
Kinetic Energy
- 42. Multiple Choice
A metal cube at temperature of 70°C is immersed in water at temperature of 20°C. The metal _______ heat while the water __________ heat.
gains, loses
loses, gains
- 43. Multiple Choice
Name the device used to measure the changes in thermal energy.
calorie
specific heat
calorimeter
styrofoam cup
- 44. Multiple Choice
If two objects have different temperatures when they come in contact, heat will flow from the warmer object to the cooler one UNTIL ____________
one reaches a temperature of zero
they both have an equal temperature
one runs out of energy
- 45. Multiple Choice
Exchange of heat in a Calorimeter depends upon
mass
difference in temperature
specific heat
none of the above
- Answer choicesTagsAnswer choicesTags