Free Printable Topic 5 Review

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Topic 5 Review

Total questions: 68

Worksheet time: 2hrs 4mins

Name

Class

Date

For the formula:
Q= m c ∆T
The units for specific heat are:

g /J C

°C/g J

kJ/g

J/g°C

What would be the effect on the particles if more heat is supplied to the system?

They would slow down

They would stop moving

They would speed up

There would be no effect

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

The total energy of all the particles in a substance is called:

temperature

thermal energy

degrees

mass

If the specific heat of water is 4.18 J/g∙°C, how much heat is required to increase the temperature of 1.2 kg of water from 23 °C to 39 °C? (show your work)

-80,256 J

80.256 J

80,256 J

-80.256 J

What is the specific heat of an unknown substance if 100.0 g of it at 200.0 °C reaches an equilibrium temperature of 27.1 °C when it comes in contact with a calorimeter of water. The water weighs 75. g and had an initial temperature of 20.00 °C? (Specific heat of water is 4.18 J/g°C) (show your work)

0.111 J/g°C

1.29 J/g°C

0.129 J/g°C

22225.85 J

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

The SI unit of heat and energy is the __________.

calorie

heat

joule

watt

A sample of iron receives 50.J of heat energy that raises the temperature of the iron by 25.0°C. If iron has a specific heat of 0.10 J/g°C, what is the mass of the iron sample? (show your work)

25g

30g

20g

50g

10.

A reaction is performed in a beaker with a temperature probe recording the temperature changes of the reaction. If the temperature began at 15.0 degrees Celsius and ended at 27.5 degrees Celsius. Is the reaction endothermic or exothermic?

Exothermic

Endothermic

11.

Calorimetry Question:
A piece of metal with a mass of 32.8 g is heated to 100.5°C and dropped into 138.2 g of water at 20.0°C. The final temperature of the system is 30.2°C. What is the specific heat capacity of the metal? (show your work)

2.56 J/g°C

0.391 J/g°C

5.29 J/g°C

3.50 J/g°C

12.

In an exothermic process, the surroundings are gaining energy.

True

False

13.

What does "q" mean?

A measure of heat energy

A change in heat energy

A measure of kinetic energy

A change in temperature

14.

What is a tool that measures the heat of chemical reactions?

calorimeter

calorie

Styrofoam™ cup

none of these

15.

Calorimeters 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.

16.

A metal cube at temperature of 10°C immersed in a liquid at temperature of 70°C.
What is the temperature of the metal cube when thermal equilibrium is achieved between the cube and the liquid?

Between 10°C and 70°C

More than 70°C

Less than 10°C

Same as the room temperature

17.

The specific heat of water is 4.18 J/g°C.

If 980. J of energy is added to 6.20 g of water at 18.0 °C, what is the final temperature of the water?

37.8 °C

-19.8 °C

19.8 °C

55.8 °C

18.

What does "ΔT" mean?

A change in health

A change in heat

A change in height

A change in temperature

19.

3 C₂H₂(g) → C₆H₆(g)

What is the standard enthalphy change ΔH^o, for the reaction represented above?

(ΔH^o_f of C₂H₂(g) is 230 kJ mol^-1;

(ΔH^o_f of C₆H₆(g) is 83 kJ mol^-1;)

-607 kJ

-147 kJ

-19 kJ

+19 kJ

+773 kJ

20.

2 NH₃(g) → 3 H₂(g) + N₂(g) ΔH°₂₉₈= 92 kJ/mol_rxn

According to the information above, what is the standard enthalpy of formation, ΔH°_f , for NH₃(g) at 298 K ?

-92 kJ/mol

-46 kJ/mol

46 kJ/mol

92 kJ/mol

184 kJ/mol

21.

Based on the information in the table above, which of the following expressions gives the approximate ΔH° for the reaction represented by the following balanced chemical equation?

Fe2O3(s)+3 CO(g)→2 Fe(s)+3 CO2(g)

ΔH°rxn=[(0kJ/mol)+(−394kJ/mol)]−[(−826kJ/mol)+(−111kJ/mol)]

ΔH°rxn=[2(0kJ/mol)+ 3(−394kJ/mol)]−[(−826kJ/mol)+ 3(−111kJ/mol)]

ΔH°rxn=[(−826kJ/mol)+ 3(−111kJ/mol)]−[2(0kJ/mol)+ 3(−394kJ/mol)]

ΔH°rxn=[(−826kJ/mol)+(−111kJ/mol)]−[(0kJ/mol)+(−394kJ/mol)]

22.

The enthalpy change for the reaction 2Al(s)+Fe2O3(s)→2Fe(s)+Al2O3(s) is −860kJ/mol. Based on the standard enthalpies of formation ΔH°f provided in the table, what is the approximate ΔH°f for Fe2O3(s) ?

+2540kJ/mol

−2540kJ/mol

+820kJ/mol

−820kJ/mol

23.

C(s)+H2O(g)→CO(g)+H2(g)

ΔH°=+131kJ/molrxn

The reaction between C(s) and H2O(g) is represented by the balanced chemical equation above. Based on the enthalpy change of the reaction (ΔH°) and the standard heats of formation (ΔH°f) given in the table below, what is the approximate ΔH°f for CO(g) ?

−373kJ/mol

−111kJ/mol

+111kJ/mol

+373kJ/mol

24.

4 NH₃(g) + 3 O₂(g) → 2 N₂(g) + 6 H₂O(g)

If the standard molar heats of formation of ammonia, NH₃(g), and gaseous water, H₂O(g), are -46 kJ/mol and -242 kJ/mol, respectively, what is the value of ΔH°₂₉₈ for the reaction represented above?

-190 kJ/mol_rxn

-290 kJ/mol_rxn

-580 kJ/mol_rxn

-1,270 kJ/mol_rxn

-1,640 kJ/mol_rxn

25.

Calculate the enthalpy of reaction (ΔH).

4CO_{2 (g)} + 6H₂O _(g) → 2C₂H_{6 (g)} + 7O_{2 (g)}

ΔH_f^o [CO_2(g)] = -393.5 kJ

ΔH_f^o[H₂O_(g)] = -241.8 kJ

ΔH_f^o [C₂H_6(g)] = -84.7 kJ

550.647 KJ/mol

2855.584 KJ/mol

-550.647 KJ/mol

-2855.584 KJ/mol

26.

The standard enthalpy changes of formation of carbon dioxide and of methanoic acid are −394 kJ/mol and −409 kJ/mol respectively. Calculate the enthalpy change for the reaction

H₂ _(g) + CO₂ _(g) → HCOOH _(l)

−803 kJ/mol

−15 kJ/mol

+803 kJ/mol

+15 kJ/mol

27.

The standard enthalpy of formation of NH₃ (g) at 298K is -46 kJmol^-1. What is the enthalpy change of the following reaction?

2NH₃(g) ---> N₂(g) + 3H₂(g)

-46 kJmol^-1

+92 kJmol^-1

-92 kJmol^-1

+46 kJmol^-1

28.

The standard enthalpies of formation for ethene (C₂H₄), water (H₂O) and ethanol (C₂H₅OH) are +52, -286 and -277 kJ/mol respectively. Calculate ∆H^o for the reaction Ethene + Water → Ethanol

+61 kJ

-43 kJ

-61 kJ

-511 kJ

-615 kJ

29.

Whenever you are looking up delta H values in a table, does the state of the element/compound matter?

Yes, always

No, Never

Only if it is a solid

It is always zero

30.

Which is expected NOT to have a $\Delta H_f^{\degree}$ value of zero?

F₂(g)

Br₂(g)

I₂(s)

C(s, graphite)

31.

When finding the enthalpy change from enthalpies of formation, the formula is...

$\Delta H\ =\ \sum_{ }^{ }\Delta H_{products\ }-\ \sum_{ }^{ }\Delta H_{reac\tan ts\ }$

$\Delta H\ =\ \sum_{ }^{ }\Delta H_{reac\tan ts\ }-\ \sum_{ }^{ }\Delta H_{products\ }$

32.

When calculating enthalpy change from enthalpy of formation,

multiply the H_f for each compound by the subscript

multiply the H_f for each compound by the coefficient

33.

The reaction represented goes essentially to completion. The reaction takes place in a rigid, insulated vessel that is initially at 600 K

Which of the following statements about the bonds in the reactants and products is most accurate?

The sum of the bond enthalpies of the bonds in the reactant is greater than the sum of the bond enthalpies of the bonds in the products.

The sum of the bond enthalpies of the bonds in the reactant is less than the sum of the bond enthalpies of the bonds in the products.

The length of the bond between carbon and oxygen in CH₃OH is shorter than the length of the bond between carbon and oxygen in CO.

All of the bonds in the reactant and products are polar.

34.

Which of the following statements must be true for the combustion of CH4(g), represented by the equation? $CH_4(g)+2\ O_2(g)→CO_2(g)+2\ H_2O(g)\ \ \ \ \ \ \ \ \ \ \ \ ΔH°<0$

The bond dissociation energy between O atoms in O2 is greater than the sum of the bond dissociation energies of the two O−H bonds in H2O.

More bonds are formed in the products than are broken in the reactants.

The sum of the bond dissociation energies of the product molecules is EQUAL to the sum of the bond dissociation energies of the reactant molecules.

The sum of the bond dissociation energies of the product molecules is GREATER than the sum of the bond dissociation energies of the reactant molecules.

35.

CO(g) + 2 H₂(g) ⇄ CH₃OH(g) ΔH < 0

The synthesis of CH₃OH(g) from CO(g) and H₂(g) is represented by the equation above. The value of K_c for the reaction at 483 K is 14.5.

Which of the following statements is true about bond energies in this reaction?

The energy absorbed as the bonds in the reactants are broken is greater than the energy released as the bonds in the product are formed.

The energy released as the bonds in the reactants are broken is greater than the energy absorbed as the bonds in the product are formed.

The energy absorbed as the bonds in the reactants are broken is less than the energy released as the bonds in the product are formed.

The energy released as the bonds in the reactants are broken is less than the energy absorbed as the bonds in the product are formed.

36.

The oxidation of carbon monoxide can be represented by the chemical equation $2CO(g)+O_2(g)→2CO_2(g)$ . The table above provides the average bond enthalpies for different bond types. Based on the information in the table, which of the following mathematical expressions is correct for the estimated enthalpy change for the reaction?

$ΔHrxn=[2(1072\ \frac{kJ}{mol})+(498\ \frac{kJ}{mol})]−2(799\ \frac{kJ}{mol})$

$ΔHrxn=[2(1072\ \frac{kJ}{mol})+(498\ \frac{kJ}{mol})]−4(799\ \frac{kJ}{mol})$

$ΔHrxn=[2(799\frac{kJ}{mol})+(142\frac{kJ}{mol})]−4(360\frac{kJ}{mol})$

$ΔHrxn=[2(799\frac{kJ}{mol})+(142\frac{kJ}{mol})]−2(360\frac{kJ}{mol})$

37.

Shown above are the equation representing the decomposition of H2O2(l) and a table of bond enthalpies. On the basis of the information, which of the following is the enthalpy of decomposition of 2 mol of H2O2(l) ?

−349kJ

−203kJ

203kJ

349kJ

38.

An equation representing the dissociation of O2(g) and a table of bond enthalpies are shown above. Based on the information, which of the following is the enthalpy of dissociation for O2(g)?

−641kJ/mol

−495kJ/mol

495kJ/mol

641kJ/mol

39.

The first ionization energy of an element is the energy required to remove an electron from a gaseous atom of the element (i.e., X(g) → X⁺(g) + e⁻). The values of the first ionization energies for the third-row elements are shown in the graph above. On the basis of the information given, which of the following reactions is exothermic?

$Cl+Mg^+→\ Cl^++Mg$

$Al+Mg^+→\ Al^++Mg$

$P+Mg^+→\ P^++Mg$

$S+Mg^+→\ S^++Mg$

40.

CH₄(g) + Cl(g) → CH₃(g) + HCl(g) ΔH° = -14 kJ/mol_rxn

NH₃(g) + Cl(g) → NH₂(g) + HCl(g) ΔH° = -36 kJ/mol_rxn

H₂O(g) + Cl(g) → OH(g) + HCl(g) ΔH° = + 40 kJ/mol_rxn

Based on the data above, what can be concluded regarding the strength of the C-H, N-H, and O-H bonds in the molecules shown?

The C-H bond is the strongest.

The N-H bond is the strongest.

The O-H bond is the strongest.

Nothing can be concluded without knowing the strength of the H- Cl bond.

41.

A mixture of NO₂(g) and N₂O₄(g) is placed in a glass tube and allowed to reach equilibrium at 70°C, as represented above.

Which of the following statements about ∆H° for the reaction is correct?

ΔH° < 0 because energy is released when the N−N bond breaks.

ΔH° < 0 because energy is required to break the N−N bond.

ΔH° > 0 because energy is released when the N−N bond breaks.

ΔH° > 0 because energy is required to break the N−N bond.

42.

Based on the bond energies shown in the table above, which of the following diagrams best represents the change in energy as the reaction represented below proceeds?

H₂(g)+ Cl₂(g)→2HCl(g)

43.

_____ Hydrogen-Hydrogen single bond/s are broken and _____ Carbon-Hydrogen single bond/s formed

6; 8

2; 8

2; 10

6; 10

44.

_____ Carbon-Carbon single bond/s are formed

45.

Bond enthalpy is the amount of energy is takes to break __________ of a bond.

one mole

one gram

the activation energy

the binding energy

46.

Using bond energies to solve for enthalpy,

$\Delta H$ = Bond broken - bonds formed

undefined = Bond formed- bonds broken

undefined = products - reactants

undefined = reactants- products

47.

Some average bond enthalpies, in kJ/mol, are as follows:
H-H = 436
Cl-Cl = 242
H-Cl = 431
What is the enthalpy change for the decomposition of hydrogen chloride?
2 HCl --> H₂ + Cl₂

-184 kJ

+ 184 kJ

- 247 kJ

+ 247 kJ

48.

The average bond enthalpies for O-O and O=O are 146kJ/mol and 496kJ/mol respectively. Calculate the enthalpy change for the reaction shown.

-102kJ

+102kJ

+146kJ

-248 kJ

49.

Some average bond enthalpies, in kJ/mol, are as follows:
H-H = 436
Cl-Cl = 242
H-Cl = 431
What is the enthalpy change for the decomposition of hydrogen chloride?
2 HCl --> H₂ + Cl₂

-184 kJ

+ 184 kJ

- 247 kJ

+ 247 kJ

50.

Breaking bonds is _________________. Forming bonds is ______________________

endothermic, exothermic

exothermic, endothermic

51.

ΔH value in an endothermic reaction is a positive number.

True

False

52.

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

53.

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

54.

How do you calculate Enthalpy of a reaction?

ΔH = ΔH_products- ΔH_reactants

ΔT = q / mC

ΔG = ΔH -TΔS

E = mc²

55.

"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

56.

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.

57.

Which of the following has a ΔH_f^o value of 0?

Br₂(g)

N(g)

CO(g)

N₂(g)

58.

Which of the equation below refers to the standard enthalpy of formation, ΔH_f^o?

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

59.

Good ozone is formed in the

troposhere

stratosphere

mesosphere

thermosphere

60.

What is the name of the international agreement committing parties to phasing out ozone depleting substances and phasing out chlorofluorocarbons (CFCs)?

Vienna Protocol

Paris Agreement

Montreal Protocol

Antarctic Convention

61.

The depletion in the Ozone layer is caused by:

Carbon dioxide

Nitrous oxide

Methane

Chlorofluorocarbon

62.

Which are effects of UV radiation on living organisms? select ALL that are true.

It can cause cataracts.

It can cause mutation in DNA.

It can disrupt food chains by causing harm to photosynthetic organisms.

It can cause organisms to overheat.

63.

Which is the proper expression about OZONE?

Good Up High, Bad Nearby

Bad Up High , Good Nearby

64.

The ozone layer protects us from

Increased atmospheric heat

CFCs

UV rays

Decreased atmospheric heat

65.

The enthalpy change for the reaction, ∆H_r , is equal to

∆H₁+∆H₂

∆H₁-∆H₂

-∆H₁ -∆H₂

-∆H₁+∆H₂

66.

The enthalpy change for the reaction to form hydrated sodium thiosulfate crystals cannot be measured directly. The following Hess cycle can be used. The enthalpy change for the reaction, ΔHr, is equal to ...

ΔH₁ + ΔH₂

ΔH₁ − ΔH₂

− ΔH₁ − ΔH₂

− ΔH₁ + ΔH₂

67.

The enthalpy change associated with a reaction carried out in multiple steps is ________ the sum of the enthalpy changes for each individual step.

Greater than

Equal to

Less than

68.

which of the following enthalpy changes represent the enthalpy change of formation?

Mg(s) + Cl₂(g) → MgCl₂(s)

Mg²⁺(g) + 2 Cl ^-(g) → MgCl₂(aq)

O2(g) → 2 O(g)

2Mg (s) + O₂(g) → 2MgO(S)

100 %

Topic 5 Review

Total questions: 68

Worksheet time: 2hrs 4mins

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