Why is it when using bond enthalpies to calculate enthalpies of reaction, they are not always accurate and enthalpies of formation are preferred?
The effects of nearby atoms can strengthen or weaken any bond.
As an illustration:
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Bond enthalpies are not always accurate for calculating enthalpies of reaction because they represent average values and do not account for factors such as bond angle variations, molecular geometry, and electronic effects. Enthalpies of formation are preferred because they directly measure the energy change associated with forming one mole of a compound from its constituent elements in their standard states, providing more precise and reliable values for calculating enthalpies of reaction.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
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