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Enthalpy

Total questions: 45

Worksheet time: 49mins

Name
Class
Date
1.

How do you calculate Enthalpy of a reaction?

a)

ΔH = ΔHproducts - ΔHreactants

b)

ΔT = q / mC

c)

ΔG = ΔH -TΔS

d)

E = mc2

2.
Specific heat capacity is
a)
heat energy needed to raise temp by 1C
b)
heat energy needed to raise temp of 1g of substance by 1C
c)
heat energy absorb to raise 1g of substance to higher temp
d)
heat energy need to raise temp for 1g of substance
3.

"Heat change when 1 mole of gaseous atom is formed from its element at standard condition" is the definition for _______.

a)

standard enthalpy of formation

b)

standard enthalpy ofhydration

c)

electron affinity

d)

standard enthalpy of atomisation

4.

What is standard enthalpy of formation, ΔHfo?

a)

Heat change when 1 mole of gaseous ions is hydrated in water at 25oC and 1 atm

b)

Heat change when 1 mole of compound is formed from its elements in their stable state at standard condition of 25oC and 1 atm

c)

Heat change when 1 mole of gaseous atom is formed from its elements at 25oC and 1 atm

d)

Heat change when 1 mole of electrons is removed from 1 mole of gaseous atoms at ground state at 25oC and 1 atm

5.

Name the type of enthalpy for the following reaction:

Na+ (g) --> Na+ (aq) ΔH = -364 kJmol-1

a)

Standard enthalpy of neutralisation, ΔHneuto

b)

Standard enthalpy of solution, ΔHsolno

c)

Standard enthalpy of hydration, ΔHhydo

d)

lattice energy, ΔHlatticeo

6.

Enthalpy change represented by the equation

MgSO4 (s) ---> Mg2+ (aq) + SO4 2- (aq)

is known as_____________.

a)

ionization energy of magnesium and sulphate

b)

lattice crystal energy of magnesium sulphate

c)

enthalpy of solution of magnesium sulphate

d)

enthalpy of hydration of magnesium sulphate

7.

Define standard enthalpy of combustion.

a)

Heat released when one mole of substance is burnt completely in excess oxygen.

b)

Heat absorbed when one mole of substance is burnt completely in excess oxygen under standard conditionj

c)

Heat released when one mole of substance is burnt completely in excess oxygen under standard condition.

d)

Heat change when one mole of substance is burnt partially in excess oxygen under standard condition.

8.

Which of the following has a ΔHfo value of 0?

a)

Br2(g)

b)

N(g)

c)

CO(g)

d)

Ne(g)

9.

What is the type of standard enthalpy of this reaction?

Na(s) ---> Na(g) ΔH = +109 kJmol-1

a)

standard enthalpy of formation

b)

standard enthalpy of combustion

c)

standard enthalpy of atomisation

d)

standard enthalpy of hydration

10.

Which of the equation below refers to the standard enthalpy of formation, ΔHfo?

a)

Na(g) ---> Na+(g) + e- ΔH = -364 kJmol-1

b)

C2H5OH(l) + 3O2(g) ---> 2CO2(g) + 3H2O (l) ΔH = - 1286 kJmol-1

c)

2C(s) + 2H2(g) ---> C2H4 (g) ΔH = - 52.3 kJmol-1

d)

Na+(g) ---> Na+(aq) ΔH = - 364 kJmol-1

11.

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)?

a)

the formation of ZnO (s) is endothermic

b)

the formation of ZnO (s) is exothermic

c)

the formation of ZnO (s) does not require energy

d)

the formation of ZnO (s) absorbs heat.

12.
Which statement is true regarding endothermic reactions?
a)
a) Temperature change is positive and enthalpy change is positive
b)
b) Temperature change is positive and enthalpy change is negative
c)
c) Temperature change is negative and enthalpy change is positive
d)
d) Temperature change is negative and enthalpy change is negative
13.
Endothermic reactions feel
a)
warm
b)
cold
14.
Define 'Enthalpy'
a)
a) Energy stored in the movement of molecules in a substance
b)
b) The opposite of temperature
c)
c) The temperature of a molecule
d)
d) Energy stored in the chemical bonds in a substance
15.
Heat is measured in 
a)
joules
b)
grams
c)
degrees celcius
16.
Describe the energy change that takes place when bonds are broken. 
a)
a) Energy is given out 
b)
b) Energy is taken in 
c)
c) Energy is taken in and then given out 
d)
d) Energy is given out and then taken in
17.
Which is an example of an endothermic physical reaction? 
a)
a) Ice melting 
b)
b) Combustion 
c)
c) Steam condensing 
d)
d) Photosynthesis
18.
Calorimetry is a technique used to
a)
measure temperature change
b)
measure heat released
c)
measure heat absorbed
d)
measure the enthalpy change for a reaction
19.
Which statement is FALSE for an exothermic reaction?
a)
Reactants higher in energy and less stable
b)
Product lower in energy and more stable
c)
Products have stronger bonds than reactants
d)
Reactants have stronger bonds than products
20.

Diagram below shows

a)

lattice energy

b)

Standard enthalpy of precipitation

c)

Standard enthalpy of formation

d)

Standard enthalpy of hydration

21.

Diagram below shows

a)

Lattice energy

b)

Standard enthalpy of solution

c)

Standard enthalpy of formation

d)

Standard enthalpy of hydration

22.
ΔH value in an endothermic reaction is a positive number.
a)
True
b)
False
23.

What does the circle mean in ΔH°?

a)

Standard Conditions (T=298.15 K P=1 atm)

b)

Standard Temperature and Pressure (T=273.15 K P=1 atm)

c)

Degree K

d)

Degree C

24.
The SI unit of heat and energy is the __________.
a)
calorie
b)
heat
c)
joule
d)
watt
25.
What type of reaction is shown in the reaction pathway?
a)
endothermic reaction
b)
exothermic reaction
26.

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.

a)

The enthalpy of neutralisation

b)

The enthalpy of combustion

c)

The enthalpy of formation

d)

The enthalpy of reaction

27.

Which of the following has a ΔHfo value of 0?

a)

Br2(g)

b)

N(g)

c)

CO(g)

d)

N2(g)

28.

Define the term Exothermic by picking the correct statements

a)

Products have less energy than the reactants

b)

ΔH is negative

c)

ΔH is positive

d)

Energy is given out to the surroundings (temperature goes up).

e)

products have more energy than the reactants

29.

Define Endothermic by picking the correct statements

a)

ΔH is positive

b)

Energy is taken in from the surroundings (temperature goes down).

c)

Energy is given out to the surroundings (temperature goes up).

d)

· Products have less energy than the reactants

e)

products have more energy than the reactants

30.
Which statement is true regarding endothermic reactions?
a)
a) Temperature change is positive and enthalpy change is positive
b)
b) Temperature change is positive and enthalpy change is negative
c)
c) Temperature change is negative and enthalpy change is positive
d)
d) Temperature change is negative and enthalpy change is negative
31.

Standard enthalpy change of formation, ΔfHΘ, is the enthalpy change that takes place when one mole of a compound is formed from its (a)   under standard conditions (with all reactants and products in standard states).

32.

What value in kJ mol-1 is the standard enthalpy change of formation, ΔfHΘ, of any element?

(a)  

33.

The enthalpy of neutralisation is the enthalpy change

a)

when one mole of the pure compound is formed from its elements under standard conditions

b)

when 1 mole of pure substance is completely burned in excess oxygen, under the given temperature and pressure of the reaction

c)

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

d)

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.
 For 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 sublimates
a)
4 only
b)
1 only
c)
3 and 4 only
d)
2 and 3 only
35.

What is the name of this enthapy change

a)

Enthalpy of formation

b)

Enthalpy of combustion

c)

Enthalpy of reaction

d)

Enthalpy of atomisation

36.

Which of the following equations represents the enthalpy change of combustion?

a)

2C4H10(g) +13O2(g) → 8CO2 (g) + 10H20(g)

b)

C4H10(g) +13/2O2(g) → 4CO2 (g) + 5H20(g)

c)

C4H10 + 9/2O2 = 4CO (s)+ 5H2O

d)

C4H10 + 5/2O2 = 4C(s) + 5H2O(g)

37.
C+ O2 --> CO2 + 60kJ, what is the value for ΔH for the reaction?
a)
+60
b)
-60
c)
there is no way to know
38.

What is the standard enthalpy change of formation?

a)

2Fe (s) + 11/2O2(g) → Fe2O3(s)

b)

4Fe (s) + 3O2 → 2 Fe2O3(s)

c)

2H2(g) + O2 (g) → 2H2O (l)

39.

For a skillet, used for cooking, do you want a high or low specific heat

a)

High, so that it will need more energy to heat up

b)

Low, so that it will change temperature quickly

40.
Calorimeters use insulating materials to:
a)
encourage affordable materials in science experiments in schools.
b)
preserve the heat of the environment outside the Styrofoam cup.
c)
prevent heat from escaping to the environment.
d)
keep the liquid inside the Styrofoam cup from overheating.
41.

The amount of energy required to raise the temperature 1ºC for every gram is called____?

a)

Thermal Energy

b)

Specific Heat Capacity

c)

Temperature

d)

Kinetic Energy

42.

A metal cube at temperature of 70°C is immersed in water at temperature of 20°C. The metal _______ heat while the water __________ heat.

a)

gains, loses

b)

loses, gains

43.

Name the device used to measure the changes in thermal energy.

a)

calorie

b)

specific heat

c)

calorimeter

d)

styrofoam cup

44.

If two objects have different temperatures when they come in contact, heat will flow from the warmer object to the cooler one UNTIL ____________

a)

one reaches a temperature of zero

b)

they both have an equal temperature

c)

one runs out of energy

45.

Exchange of heat in a Calorimeter depends upon

a)

mass

b)

difference in temperature

c)

specific heat

d)

none of the above

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