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Questions and Answers
Potential Energy is energy stored in the ______ bonds of a substance.
Potential Energy is energy stored in the ______ bonds of a substance.
chemical
An endothermic reaction is a reaction where the system absorbs energy from the surrounding in the form of ______.
An endothermic reaction is a reaction where the system absorbs energy from the surrounding in the form of ______.
heat
Examples of an endothermic reaction include evaporation of ______.
Examples of an endothermic reaction include evaporation of ______.
liquid
Exothermic reaction is a reaction that releases energy from the system in the form of ______.
Exothermic reaction is a reaction that releases energy from the system in the form of ______.
Examples of an exothermic reaction include burning of a ______.
Examples of an exothermic reaction include burning of a ______.
Kinetic Energy is energy that comes from ______.
Kinetic Energy is energy that comes from ______.
The first law of thermodynamics states that energy can neither be created nor destroyed but can only changed from one form to another. Heat (q) and work (w) are the only possible forms of energy transfer, this can attribute to the overall change in energy (E) of a system. So, we can write, - The change in energy is always defined as the difference between the final state and the initial state. It is a physical property of a material that measures how much heat is required to raise the temperature of one mole of that material to 1degC.
The first law of thermodynamics states that energy can neither be created nor destroyed but can only changed from one form to another. Heat (q) and work (w) are the only possible forms of energy transfer, this can attribute to the overall change in energy (E) of a system. So, we can write, - The change in energy is always defined as the difference between the final state and the initial state. It is a physical property of a material that measures how much heat is required to raise the temperature of one mole of that material to 1degC.
Energy is transferred into a system. Work is done on a system.
Energy is transferred into a system. Work is done on a system.
A process of measuring the amount of heat released or absorbed during a chemical reaction. It can determine whether the reaction is exothermic or endothermic.
A process of measuring the amount of heat released or absorbed during a chemical reaction. It can determine whether the reaction is exothermic or endothermic.
______ is a measure of the total energy in a system/reaction. It is the total heat absorbed or released in the system. Sometimes referred to as “heat content.” The heat flow of the reaction system is equal to the difference in enthalpy between products and reactant.
______ is a measure of the total energy in a system/reaction. It is the total heat absorbed or released in the system. Sometimes referred to as “heat content.” The heat flow of the reaction system is equal to the difference in enthalpy between products and reactant.
A chemical equation that shows enthalpy relation between products and reactants. It must contain a balanced chemical equation, and the appropriate value and for change in enthalpy.
A chemical equation that shows enthalpy relation between products and reactants. It must contain a balanced chemical equation, and the appropriate value and for change in enthalpy.
The sign of change in enthalpy indicates whether the reaction, when carried out at constant pressure, is endothermic (positive change in enthalpy) or exothermic (negative change in enthalpy).
The sign of change in enthalpy indicates whether the reaction, when carried out at constant pressure, is endothermic (positive change in enthalpy) or exothermic (negative change in enthalpy).
The magnitude of change in enthalpy is directly proportional to the amount of reactant or product.
The magnitude of change in enthalpy is directly proportional to the amount of reactant or product.
Change in enthalpy for a reaction is equal in magnitude but opposite in sign to change in enthalpy for the reverse reaction.
Change in enthalpy for a reaction is equal in magnitude but opposite in sign to change in enthalpy for the reverse reaction.
The value quoted for change in enthalpy applies when the products and reactants are at the same temperature, ordinarily taken to ______ unless specified otherwise.
The value quoted for change in enthalpy applies when the products and reactants are at the same temperature, ordinarily taken to ______ unless specified otherwise.
Change in enthalpy is the same whether it occurs in one step or in a series of steps.
Change in enthalpy is the same whether it occurs in one step or in a series of steps.
Flashcards
Potential Energy
Potential Energy
Energy stored in the chemical bonds of a substance.
Kinetic Energy
Kinetic Energy
Energy arising from the motion of particles within a system.
Endothermic Reaction
Endothermic Reaction
A reaction that absorbs energy from the surroundings, typically in the form of heat.
Exothermic Reaction
Exothermic Reaction
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First Law of Thermodynamics
First Law of Thermodynamics
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Heat (q)
Heat (q)
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Work (w)
Work (w)
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Change in Energy (ΔE)
Change in Energy (ΔE)
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Specific Heat Capacity
Specific Heat Capacity
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Calorimetry
Calorimetry
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Enthalpy (H)
Enthalpy (H)
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Enthalpy Change (ΔH)
Enthalpy Change (ΔH)
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Standard Conditions for ΔH
Standard Conditions for ΔH
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Reverse Reaction Enthalpy
Reverse Reaction Enthalpy
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Enthalpy Change and Multiple Steps
Enthalpy Change and Multiple Steps
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Balanced Chemical Equation and Enthalpy
Balanced Chemical Equation and Enthalpy
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Study Notes
Potential and Kinetic Energy
- Potential Energy is stored in the chemical bonds of a substance.
- Kinetic Energy arises from the motion of particles within a system.
Endothermic and Exothermic Reactions
- Endothermic reactions absorb energy from the surroundings in the form of heat.
- An example of an endothermic reaction includes the evaporation of water.
- Exothermic reactions release energy, typically as heat.
- An example of an exothermic reaction is the burning of a fuel.
Thermodynamics Principles
- The first law of thermodynamics asserts that energy cannot be created or destroyed, only transformed.
- Heat (q) and work (w) are the only forms of energy transfer affecting a system's energy change (ΔE).
- The change in energy is defined as the difference between the final state and the initial state of the system.
Measuring Heat and Enthalpy
- Specific heat capacity measures heat required to raise the temperature of one mole of a material by 1°C.
- Energy can be transferred into a system as work is done on it.
- Calorimetry is used to measure the amount of heat released or absorbed during a chemical reaction, determining if it is endothermic or exothermic.
- Enthalpy (H) is the total energy in a system or reaction, also known as "heat content."
Enthalpy Changes
- The heat flow of a reaction is equal to the difference in enthalpy between products and reactants.
- A balanced chemical equation is necessary to describe the enthalpy relationship effectively, including the change in enthalpy (ΔH).
- The sign of ΔH indicates the nature of the reaction: positive for endothermic and negative for exothermic.
- The magnitude of ΔH is proportional to the quantity of reactants or products involved.
- ΔH is equal in magnitude but opposite in sign for the reverse reaction.
- Standard conditions for quoting ΔH are at the same temperature, usually 25°C unless stated otherwise.
- The change in enthalpy remains consistent regardless of whether a reaction occurs in one step or multiple steps.
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Description
Test your knowledge of thermodynamics and energy in chemistry with this review quiz for engineering students. Topics include potential energy, endothermic reactions, and more.
