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Gas Test Review

Gas Laws & Collision Theory

QuestionAnswer
Gas Laws Boyle's law , Charles law, gay-lussacs law,combined gas laws,ideal gas laws
example of Boyles law inflating a balloon
example of Charles law heating a sealed container
4 properties that can help you predict the behavior of gases pressure,volume,temperature,number of moles
Boyles law the inverse relationship between the pressure and volume of a gas,when the temperature is held constant
Charles law the direct relationship between the volume and temperature of a gas,when pressure is held constant
gay;Lussac law the direct relationship between the pressure and temperature of a gas when volume is held constant
combining the laws the law that combines Boyles,Charles,and gay-lussacs laws
ideal gas law the law that combines the four properties predicting the behavior of gases is the ideal gas law
Collision Theory: rate of reaction refers to how quickly reactants are transformed into products in a chemical reaction. the change of reactant and products per unit time
change in concentration over time Monitoring the decrease in concentration of reactants or increase in concentration of products over a specific period.
change in mass over time Measuring the loss of mass due to the release of gas or gain of mass due to the formation of a solid.
Collision Theory chemical reactions occur when reactant molecules collide with sufficient energy and with the proper orientation.
two conditions for an effective collision Energy: Colliding particles must possess enough kinetic energy to overcome the activation energy barrier. Orientation: Collisions must occur with the correct spatial orientation to allow for effective bonding and reaction.
can collision occur where there is no reaction yes
What is the minimum amount of energy needed for the particles to react? Is it different for each reaction? The minimum amount of energy required for particles to react is called the activation energy (Ea). It varies for each reaction and depends on the specific molecular structure and reaction conditions.
temperature Temperature: Increasing temperature generally speeds up reactions by providing more kinetic energy to reactant molecules.
concentration Concentration: Higher concentrations of reactants typically lead to more frequent collisions and increased reaction rates.
surface area Surface Area: In reactions involving solids, increasing the surface area of solid reactants exposes more particles to potential collisions, thereby increasing the rate.
catalysts Catalysts provide an alternative reaction pathway with lower activation energy, speeding up the reaction without being consumed themselves.
pressure Increasing pressure can accelerate reactions involving gases by decreasing the volume and increasing the frequency of collisions between gas molecules.
Created by: Silvann1e.08
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