Question

Indicate whether each statement is true or false. If it is false, rewrite it so that it is true. (a) If you measure the rate constant for a reaction at different temperatures, you can calculate the overall enthalpy change for the reaction. (b) Exothermic reactions are faster than endothermic reactions. (c) If you double the temperature for a reaction, you cut the activation energy in half.

Short answer

(a) False. If you measure the rate constant for a reaction at different temperatures, you can calculate the activation energy for the reaction, which can then be used, along with reaction enthalpies, to calculate the overall enthalpy change for the reaction. (b) False. Exothermic reactions can be faster than endothermic reactions under certain conditions, but the speed of a reaction depends on multiple factors, including activation energy, reaction mechanism, temperature, and concentration of reactants. (c) False. The relationship between temperature and activation energy is defined by the Arrhenius equation, which shows that increasing the temperature can increase the reaction rate. However, doubling the temperature does not directly cause the activation energy to be cut in half.

Step-by-step solution

Statement (a) Analysis

The statement says that the rate constant for a reaction at different temperatures can be used to calculate the overall enthalpy change for the reaction. This statement is false because the rate constant can't be directly used to find the overall enthalpy change. However, using the Arrhenius equation, a relationship between rate constants at different temperatures and activation energy can be obtained. Once we have the activation energy, we can use it along with the reaction enthalpies to calculate the overall enthalpy change.

Rewrite Statement (a)

If you measure the rate constant for a reaction at different temperatures, you can calculate the activation energy for the reaction, which can then be used, along with reaction enthalpies, to calculate the overall enthalpy change for the reaction.

Statement (b) Analysis

The statement says that exothermic reactions are faster than endothermic reactions. This is a false statement because the speed of a reaction depends on many factors like activation energy, reaction mechanism, temperature, and concentration of reactants. While it is generally believed that exothermic reactions can be faster due to the release of energy, it's not always the case.

Rewrite Statement (b)

Exothermic reactions can be faster than endothermic reactions under certain conditions, but the speed of a reaction depends on multiple factors, including activation energy, reaction mechanism, temperature, and concentration of reactants.

Statement (c) Analysis

The statement says that if you double the temperature for a reaction, you cut the activation energy in half. This statement is false. Temperature and activation energy have a complex relationship defined by the Arrhenius equation, and doubling the temperature does not necessarily cut the activation energy in half.

Rewrite Statement (c)

The relationship between temperature and activation energy is defined by the Arrhenius equation, which shows that increasing the temperature can increase the reaction rate. However, doubling the temperature does not directly cause the activation energy to be cut in half.

Key concepts

Rate Constant

The rate constant is a vital component in the study of reaction kinetics. It represents the speed at which a chemical reaction occurs. Imagine it as a measure of how quickly reactants are converted into products. The rate constant is denoted by the symbol \(k\). Its value can change with temperature, which makes it unique to each reaction under certain conditions.

Several factors can influence the rate constant:

• Temperature: Typically, as the temperature rises, the rate constant increases, resulting in a faster reaction.
• Nature of Reactants: Different reactants have different reactivities, affecting the rate constant.
• Catalysts: A catalyst can lower the activation energy, thereby increasing the rate constant.

When calculated accurately, the rate constant provides insights into the reaction mechanism and the kinetic behavior of the system.

It's important to remember that while the rate constant tells us about reaction speed, it alone can't determine enthalpy change or whether a reaction is exothermic or endothermic.

Activation Energy

Activation energy is the minimum amount of energy needed for a reaction to occur. It acts like a barrier that reactants must overcome to transform into products. Think of it as the energy "hurdle" that must be cleared for a chemical process to proceed.

Activation energy is crucial because:

• Determines Reaction Rates: Reactions with lower activation energies proceed faster compared to those with high activation energies.
• Influences Temperature Dependence: As temperature increases, more molecules have the necessary energy to surmount the activation energy barrier, thus increasing the reaction rate.

To find the activation energy, we can use the Arrhenius equation by observing how the rate constant changes at different temperatures. Activation energy is not reduced by simply doubling the temperature; rather, it remains constant for a given reaction under specific conditions.

Enthalpy Change

Enthalpy change refers to the overall energy change in a chemical reaction. It indicates whether a reaction absorbs or releases heat. This concept is essential as it defines the thermodynamic nature of a reaction.

Types of enthalpy changes include:

• Exothermic Reactions: These release energy, usually in the form of heat, making them feel warm. For example, combustion reactions often have negative enthalpy changes.
• Endothermic Reactions: These absorb energy from their surroundings, often leading to a decrease in temperature. Photosynthesis is a classic example, with a positive enthalpy change.

Enthalpy change can be computed using calorimetry or calculated from known enthalpies of formation. While the rate constant and the activation energy contribute to understanding reaction kinetics, enthalpy change provides insight into the conservation and transformation of energy during the reaction.

Arrhenius Equation

The Arrhenius equation is a key formula in chemical kinetics that relates the rate constant \(k\) to temperature \(T\) and activation energy \(E_a\). It provides a mathematical framework to explain how changes in temperature impact reaction rates. The equation is expressed as:\[k = A e^{-E_a/(RT)}\]where:

• \(A\) is the pre-exponential factor, a constant specific to each reaction.
• \(E_a\) is the activation energy.
• \(R\) is the universal gas constant \(8.314 \, J/mol \cdot K\).
• \(T\) is the temperature in Kelvin.

This equation demonstrates that with an increase in temperature, the rate constant \(k\) increases exponentially. Consequently, the reaction rate rises. Note that the Arrhenius equation sets the stage for understanding the complex relationship between temperature and activation energy, clarifying why increasing temperature can lead to faster reactions. It also underscores why doubling temperature doesn't halve the activation energy—it enhances kinetic energy, allowing more molecules to overcome existing activation energy barriers.