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Explain in your own words the difference between a spontaneous reaction and one that occurs instantaneously. a. A spontaneous reaction is one which releases free energy and moves to a more stable state. Instantaneous reactions occur rapidly with sudden release of energy. b. A spontaneous reaction is one which utilizes free energy and moves to a more stable state. Instantaneous reactions occur rapidly with sudden release of energy. c. A spontaneous reaction is one which releases free energy and moves to a more stable state. Instantaneous reactions occur rapidly within a system by uptake of energy. d. A spontaneous reaction is one in which the reaction occurs rapidly with sudden release of energy. Instantaneous reaction releases free energy and moves to a more stable state.

Step by step solution

01

Identify the Definitions

Understand the definition of a spontaneous reaction: A spontaneous reaction is one where the process occurs without continuous input of energy and moves towards a more stable state, typically releasing free energy. Additionally, understand that an instantaneous reaction occurs very quickly, often with a sudden release of energy.

02

Analyze Option A

Option A states that a spontaneous reaction releases free energy and moves to a more stable state, and an instantaneous reaction occurs rapidly with sudden release of energy. This is correct.

03

Analyze Option B

Option B states that a spontaneous reaction utilizes free energy and moves to a more stable state, which is incorrect because a spontaneous reaction releases free energy.

04

Analyze Option C

Option C states that an instantaneous reaction occurs rapidly within a system by uptake of energy, which is incorrect. Instantaneous reactions typically involve a sudden release of energy.

05

Analyze Option D

Option D states that a spontaneous reaction occurs rapidly with sudden release of energy, which is incorrect because a spontaneous reaction is not necessarily fast. Moreover, it states that an instantaneous reaction releases free energy and moves to a more stable state, which is also incorrect.

06

Select the Correct Answer

Based on the analysis, Option A is the correct statement.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Free Energy

Free energy is a crucial concept in chemistry, particularly in understanding reactions. In simple terms, it's the energy available to do work in a system. Free energy changes (ΔG) indicate whether a reaction is spontaneous or non-spontaneous.
If ΔG is negative, the reaction is spontaneous; this means it can occur without needing extra energy input.
For example, rusting of iron is a spontaneous reaction since it proceeds without continuous energy from outside.
If ΔG is positive, the reaction is non-spontaneous, indicating that external energy is necessary for the reaction to proceed.
A good real-life example is photosynthesis in plants, where sunlight (external energy) is required to convert carbon dioxide and water into glucose and oxygen.

Reaction Stability

Reaction stability refers to the final state of the products as compared to the reactants.
In a spontaneous reaction, the products are usually more stable than the reactants.
This stability is often achieved by the release of free energy, which makes the system more stable.
For instance, when gasoline burns in a car engine, the resulting carbon dioxide and water are more stable than the original gasoline.
The reaction naturally moves to this stable state without needing extra energy, making the products much less likely to react further compared to the starting materials.

Reaction Speed

Reaction speed, or reaction rate, indicates how fast a reaction occurs.
It's important to note that spontaneous doesn't mean fast.
Some spontaneous reactions can be very slow. For instance, diamond turning into graphite is spontaneous but occurs over millions of years.
On the other hand, instantaneous reactions are incredibly fast, often happening in milliseconds.
Examples include the explosion of fireworks, where chemical reactions occur almost immediately, producing a sudden burst of energy like light and heat.
Whether a reaction is spontaneous or not doesn't directly correlate with how quickly it happens.

Energy Release

Energy release is a common trait of both spontaneous and instantaneous reactions.
In a spontaneous reaction, the system loses free energy to become more stable.
This release often occurs in the form of heat, making the surroundings warmer. An example is the combustion of natural gas, which releases heat energy.
In an instantaneous reaction, the release of energy happens very quickly, often in an explosive manner.
An example is the detonation of TNT (trinitrotoluene), where a vast amount of energy is released in a very short time, causing an explosion.
The key difference is the speed of the energy release: slow and steady in spontaneous reactions, rapid and immediate in instantaneous reactions.