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IB Chemistry Topic R1.2 Energy Cycles in Reactions… | RevisionDojo

IB
R1.2 Energy cycles in reactions

S1.1 Introduction to the particulate nature of matter

S1.2 The nuclear atom

S1.3 Electron configurations

S1.4 Counting particles by mass: The mole

S1.5 Ideal gases

S2.1 The ionic model

S2.2 The covalent model

S2.3 The metallic model

S2.4 From models to materials

S3.1 The periodic table: Classification of elements

S3.2 Functional groups: Classification of organic compounds

R1.1 Measuring enthalpy change

R1.2 Energy cycles in reactions

R1.3 Energy from fuels

R1.4 Entropy and spontaneity (HL)

R2.1 How much? The amount of chemical change

R2.2 How fast? The rate of chemical change

R2.3 How far? The extent of chemical change

R3.1 Proton transfer reactions

R3.2 Electron transfer reactions

R3.3 Electron sharing reactions

R3.4 Electron-pair sharing reactions

IB Chemistry R1.2 Energy Cycles in Reactions Questionbank

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IB Chemistry Topic R1.2 Energy Cycles in Reactions Questionbank

Practice IB Chemistry Topic R1.2 Energy Cycles in Reactions with authentic exam-style questions for both SL and HL students. This question bank focuses on the exact syllabus content for R1.2 Energy Cycles in Reactions and mirrors Paper 1A, 1B, 2 style where relevant.

Get instant solutions, detailed explanations, and build confidence with questions aligned to IB examiner expectations.

Paper

Level

Difficulty

Question

HLPaper 1AFoundational

Which of the following best describes the enthalpy change when 1 mol of substance is completely burned in oxygen under standard conditions?

Question

HLPaper 1AStandard

The standard enthalpy of formation of ethanol is $-277\ \text{kJ mol}^{-1}$ . What does this value represent?

SL & HLPaper 1AStandard

Question 4HLPaper 2

Born-Haber cycles are used to calculate lattice enthalpy of N a C l . Given: Δ H_{f}^{\circ} = - 411 kJ mo l^{- 1} Sublimation of Na: + 108 Ionization energy Na: + 496 Bond enthalpy C l_{2} : + 243 Electron affinity Cl: - 349 \dots

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SL & HLPaper 1AFoundational

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2

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Which of the following statements regarding energy cycles in reactions is correct?

What statement best describes Hess's law?

Standard enthalpy of formation

Standard enthalpy of combustion

Bond enthalpy

Standard enthalpy of neutralization

Energy needed to vaporize 1 mol of ethanol

Energy released when ethanol combusts completely in oxygen

Energy required to break all bonds in 1 mol of ethanol

Energy change when 1 mol of ethanol is formed from its elements in their standard states

3

5

82

The enthalpy change for a reaction is the same regardless of the pathway taken.

The activation energy of a reaction is the same for both exothermic and endothermic reactions.

In an energy cycle, the reactants must always have a higher enthalpy than the products.

The enthalpy of formation is always a negative value.

The energy required to break chemical bonds

The enthalpy change of a reaction is independent of the route taken

The total entropy of a system must increase

The temperature change is directly proportional to mass