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Thermochemical

Total questions: 20

Worksheet time: 58mins

Name
Class
Date
1.

ΔH is the same thing as:

a)

temperature

b)

q

c)

m

d)

C

2.

ΔH means:

a)

temperature

b)

calorimetry

c)

enthalpy

d)

syntropy

3.

A positive ΔH means the reaction is:

a)

complete

b)

at equilibrium

c)

exothermic

d)

endothermic

4.

A positive ΔH means that:

a)

In order for the reaction to happen, heat must be input. It is exothermic

b)

In order for the reaction to happen, heat must be input. It is endothermic.

c)

When the reaction happens, heat is released. It is exothermic

d)

When the reaction happens, heat is released. It is endothermic

5.

If ΔH is positive, heat would be shown on the _____ side of the thermochemical equation.

a)

Reactant

b)

Product

6.
What type of reaction is shown in the reaction pathway?
a)
endothermic reaction
b)
exothermic reaction
7.

Is the following exothermic or endothermic?

a)

Endothermic

b)

Exothermic

8.

Is the following exothermic or endothermic?

a)

Endothermic

b)

Exothermic

9.
C+ O2 --> CO2 + 60kJ, what is the value for ΔH for the reaction?
a)
+60
b)
-60
c)
there is no way to know
10.

Calculate ΔH when 2 moles of ethanol (C2H5OH) reacts with excess oxygen according to the following thermochemical equation?

C2H5OH + 3O2 → 2CO2 + 3H2O ΔH = −1366.7 kJ

a)

-2733.4 kJ

b)

-683.35 kJ

c)

-1366.7 kJ

d)

-910.67 kJ

11.

What will ΔH be if there is 1 mole of oxygen?

4Fe(s) + 3O2(g) --> 2Fe2O3(s) ΔH = –1500 kJ

a)

-500 kJ

b)

500 kJ

c)

-750 kJ

d)

-4500 kJ

12.

What is ΔH if 2 mol of O2(g) is reacted in this reaction?

H2(g) + ½ O2(g) → H2O(l) ∆H = -285.8 kJ

a)

-570 kJ

b)

-71.45 kJ

c)

-1143.2 kJ

d)

-142.9 kJ

13.

What mass of P4 must be reacted to produce 5905 kJ of energy?

P4 + 6Cl2 --> 4PCl3 + 2439 kJ

a)

25.43 g

b)

563.0 g

c)

2.421 g

d)

300.0 g

14.

The enthalpy change for the reaction

C(s, graphite) + 1⁄2O2(g) --> CO(g) cannot be measured directly since some carbon dioxide is always formed in the reaction.

It can be calculated using Hess’s Law and the enthalpy changes of combustion of graphite and of carbon monoxide.


C(s, graphite) + O2(g) --> CO2 ΔH=-394 kJmol–1

CO(g) + 1⁄2O2(g) --> CO2 ΔH=-283 kJmol–1


The enthalpy change for the reaction of graphite with oxygen to give carbon monoxide is

a)

-677 kJmol–1

b)

+111 kJmol–1

c)

-111 kJmol–1

d)

+677 kJmol–1

15.
The enthalpies of combustion of C(s), H2(g) and C4H9OH(l) (in kJmol-1) are as follows  
C(s) + O2(g)   ->  CO2(g)                                               ∆H=a
H2(g) + ½O2(g)   ->   H2O(l)                                        ∆H=b
C4H9OH(l) + 6O2(g)   ->   4CO2(g) + 5H2O(l)  ∆H=c
What is the enthalpy change for the reaction shown below?
  4C(g) + 5H2(l) + ½O2(g)   ->   C4H9OH(l)
a)
c – 4a – 5b
b)
2a + 10b - c
c)
4a + 5b - c
d)
2a + 5b + c
16.

The standard enthalpy changes of combustion of carbon, hydrogen and methane are shown in the table.

Which one of the following expressions gives the correct value for the standard enthalpy change of formation of methane in kJ mol–1?

C(s) + 2H2(g) → CH4(g)

a)

394 + (2 × 286) – 891

b)

–394 – (2 × 286) + 891

c)

394 + 286 – 891

d)

–394 – 286 + 891

17.
Refer to the following question:
2N2 + 3H2 --> 2NH3 + 46 kJ
How much energy would be produced if only 1 mol of nitrogen was reacted?
a)
92 kJ
b)
0.143 kJ
c)
23 kJ
d)
15 kJ
18.
Given the following data: ΔH○f[FeO(s)] = –270kJmol–1
ΔH○f [Fe2O3(s)] = –820 kJ mol–1
Select the expression which gives the enthalpy change, in kJ mol–1, for the reaction:
2FeO(s) + 1⁄2O2(g) → Fe2O3(s) 
a)
(–820 × 1⁄2) + 270 = –140
b)
(+820 × 1⁄2) – 270 = +140
c)
–820 + (270 × 2) = –280 
d)
+820 – (270 × 2) = +280 
19.
The standard enthalpy changes of formation of iron(II) oxide, FeO(s), and aluminium oxide, Al2O3(s), are –266 kJ mol–1 and –1676 kJ mol–1 respectively.
What is the enthalpy change under standard conditions for the following reaction?
3FeO(s) + 2Al (s)   ->   3Fe(s) + Al2O3(s) 
a)
+878kJ 
b)
–878kJ 
c)
–1942kJ 
d)
–2474kJ 
20.
C2H4(g) + H2(g)   ->   C2H6(g)  ∆H°=-137 kJ mol-1
Which statement about this information is correct?
a)
The total energy of the bonds broken in the reactants is greater 
than the total energy of the bonds 
formed in the product 
b)
The bonds broken and the bonds made are of the same strength 
c)
The total energy of the bonds broken in the reactants is less than the total energy of the bonds formed in the product 
d)
No conclusion can be made about the sums of the bond enthalpies in the product compared with the reactants 

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