Free Printable IB Thermochemistry review

1.

SL: When a reaction is endothermic, ΔH is 1 and heat is 2 by the system.

a)

1: negative 2: released

b)

1: negative 2: absorbed

c)

1: positive 2: absorbed

d)

1: positive 2: released

2.

SL

a)

$1072+\left(2\times-296\right)-394$

b)

$-1072-296-394$

c)

$-1072+\left(2\times-394\right)+296$

d)

$\frac{\left(1072-394\right)}{2}+\left(-296\right)$

3.

SL

a)

$38\ kJ$

b)

$-38\ kJ$

c)

$0\ kJ$

d)

$46\ kJ$

4.

SL _____________: the enthalpy change required to break one mole of particular bonds in gaseous molecules.

a)

enthalpy of formation

b)

enthalpy of atomisation

c)

average bond enthalpy

d)

lattice enthalpy

5.

SL: The standard enthalpy of formation

( $\Delta H_f^o$ ) of liquid water is zero.

a)

True

b)

False

6.

SL: The standard enthalpy of formation

( $Δ H_{f}^{o}$ ) of gaseous water is zero.

a)

True

b)

False

7.

SL: The standard enthalpy of formation

( $Δ H_{f}^{o}$ ) of gaseous $O_2$ is zero.

a)

True

b)

False

8.

HL: The enthalpy change when one mole of gaseous ions is surrounded by water molecules to produce a solution of infinite dilution at 298 K and 100 kPa.

a)

Standard enthalpy of hydration

b)

Standard enthalpy of solution

c)

Lattice enthalpy

d)

Standard enthalpy of atomisation

9.

The enthalpy change when one mole of an ionic compound is broken into its constituent gaseous ions at 298 K and 100 kPa.

a)

Standard enthalpy of hydration

b)

Standard enthalpy of solution

c)

Lattice enthalpy

d)

Standard enthalpy of atomisation

10.

Which of the following represents the second ionisation energy of Ca.

a)

Ca_(s) → Ca²⁺_(g) + 2 e⁻

b)

Ca_(g) → Ca²⁺_(g) + 2 e⁻

c)

Ca⁺_(s) → Ca²⁺_(g) + e⁻

d)

Ca²⁺_(g) + 2 e⁻ → Ca_(s)

11.

Which of the following equations represents the C−Cl bond enthalpy in CH₃Cl?

a)

Cl_2(g) → 2 Cl_(g)

b)

CH₃Cl_(g) → CH_3(g)+ Cl_(g)

c)

CH₃Cl_(l) → CH_3(g)+ Cl_(g)

d)

CH₃Cl_(g) → CH₃⁺_(g)+ Cl^-_(g)

12.

a)

$2523kJ\ mol^{-1}$

b)

$-2523kJ\ mol^{-1}$

c)

$-2872\ kJ\ mol^{-1}$

d)

$2872\ kJ\ mol^{-1}$

13.

Which of the following show an increase in entropy? Select all correct answers.

a)

H₂O_(g)→ H₂O_(l)

b)

NaCl_(s) → Na⁺_(ag) + Cl⁻_(aq)

c)

2C₄H_{10 (g)} + 13 O₂ _(g) → 8 CO₂ _(g) + 10 H₂O _(l)

d)

CaCO₃ _(s) → CaO_(s) + CO₂ _(g)

14.

Which combination of ΔH ^θand ΔS ^θ will result in a non-spontaneous reaction at all temperatures?

a)

Positive, positive

b)

Positive, negative

c)

Negative, negative

d)

Negative, positive

15.

a)

T > 1,114K

b)

T > 298K

c)

T > 854K

d)

At all temperatures

IB Thermochemistry review

Total questions: 15

Worksheet time: 19mins

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