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Chemistry Chapter 8 : Topic 6
Reaction Pathway Diagrams
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A reaction pathway diagram shows reactants at higher energy level than products. Which conclusion is correct?
Reasoning: In exothermic reactions, reactants have higher energy than products, and excess energy is released.
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In a reaction pathway diagram, the vertical distance between reactants and products represents:
Reasoning: The energy difference between reactants and products is the enthalpy change (ΔH).
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In an endothermic reaction, which statement is correct?
Reasoning: Endothermic reactions absorb energy, so products lie at higher energy level.
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Activation energy in a reaction pathway diagram is best described as:
Reasoning: Activation energy is the energy needed to initiate a chemical reaction.
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A catalyst affects the reaction pathway diagram by:
Reasoning: A catalyst provides an alternate pathway with lower activation energy.
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Which statement about a catalyst is correct?
Reasoning: A catalyst speeds up reaction by lowering activation energy without changing (ΔH).
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In a reaction pathway diagram, the peak represents:
Reasoning: The highest point is the unstable activated complex.
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If a reaction has ΔH=+ 50 kJ, the reaction is:
Reasoning: Positive ΔH means energy is absorbed ⟹ endothermic reaction.
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Which diagram feature remains unchanged when a catalyst is used?
Reasoning: Catalysts do not affect energy difference between reactants and products.
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In an exothermic reaction pathway diagram, the energy of products is:
Reasoning: Energy is released, so products have lower energy.
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A reaction pathway shows two curves: one higher peak and one lower peak. The lower peak represents:
Reasoning: Catalyst lowers activation energy, producing a lower peak.
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What does ΔH represent in a reaction diagram?
Reasoning: ΔH is the net enthalpy change between reactants and products.
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In which case is activation energy highest?
Reasoning: Without a catalyst, more energy is needed to reach transition state.
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A student interprets a diagram where reactants and products are at the same energy level. The reaction is:
Reasoning: Equal energy means no net energy change.
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Why does a catalyst increase reaction rate?
Reasoning: Lower activation energy means more successful collisions per second.
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In an endothermic reaction pathway diagram, the correct energy trend is:
Reasoning: Energy is absorbed, so products are at higher energy level.
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The difference between peak energy and reactants energy represents:
Reasoning: This is the energy required to reach transition state.
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Which of the following does NOT change when a catalyst is added?
Reasoning: ΔH depends only on initial and final states, not pathway.
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In an exothermic reaction diagram, energy released is shown by:
Reasoning: Downward difference indicates energy release.
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A reaction has a very high peak in its energy profile. This indicates:
Reasoning: High activation energy means fewer successful collisions ⟹ slower reaction.
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