Gas Laws, Reaction Rates, and Equilibrium

Flashcards covering gas laws, collision theory, reaction rates, and equilibrium concepts.

What are the four Gas Law variables?

Temperature (T), Volume (V), Number of particles (n), and Pressure (P)

In the context of gas laws, what does temperature (T) represent?

Average kinetic energy of particles

In the context of gas laws, what is represented by volume (V)?

The space occupied by gas particles

In the context of gas laws, what does the number (n) represent?

Moles of particles, how many particles

In the context of gas laws, what does pressure (P) represent?

The force of collisions that particles experience

What is the relationship between pressure and collisions?

Higher pressure means more/stronger collisions; lower pressure means less/weaker collisions

What is the value of pressure at sea level?

1 atm

What is the relationship between Volume and Number of particles, when Temperature and Pressure are constant?

Direct

What three things are required for collision theory reactions to occur?

Reactant particles must collide, in the correct position, with enough energy to break bonds and form new ones.

Define 'reaction rate'.

Speed of a reaction = #reactions per unit of time; how fast reactants turn into products

List four factors that affect reaction rate

Temperature, mixing, surface area, and concentration and catalyst

How does increasing temperature affect reaction rate?

Increases the speed of particles, leading to more collisions and increased rate

How does mixing affect reaction rate?

Adding energy by doing work, leads to more collisions and increased rate of reaction

How does increasing surface area affect reaction rate?

More exposure leads to more contact and more collisions

How does increasing the concentration of reactants affect reaction rate?

More particles in less space leads to more collisions

How does a catalyst affect reaction rate?

Lowers activation energy by providing another path.

What is a reversible reaction?

Reactants create products at the same time as products create reactants, indicated by a double arrow.

Define dynamic equilibrium.

Rate of forward reaction = rate of reverse reaction; concentration of reactants/products is stable, particles are moving, and reactions are still happening.

What is Le Chatelier's Principle?

If a system at equilibrium is changed, it will shift to a new equilibrium to counteract the change.

What occurs when the forward reaction is faster before reaching equilibrium?

The equilibrium shifts right, and the forward reaction is favored (R → P).

What occurs when the reverse reaction is faster before reaching equilibrium?

The equilibrium shifts left, and the reverse reaction is favored (R ← P).

How does adding reactants affect equilibrium?

More reactants collide, the forward reaction is faster, and the equilibrium shifts right.

How does removing reactants affect equilibrium?

Less reactants collide, the forward reaction is slower, and the equilibrium shifts left.

How does adding products affect equilibrium?

More products collide, the reverse reaction is faster, and the equilibrium shifts left.

How does removing products affect equilibrium?

Less products collide, the reverse reaction is slower, and the equilibrium shifts right.

How does increasing temperature (adding heat) affect equilibrium?

The system will try to get rid of the added heat, favoring the endothermic reaction.

How does decreasing temperature (removing heat) affect equilibrium?

The system will try to make more heat, favoring the exothermic reaction.

How does decreasing volume (increasing pressure) affect equilibrium for gases?

The system tries to make it less to balance it, shifting to the side with less moles of gas.

How does increasing volume (decreasing pressure) affect equilibrium for gases?

The system shifts to the side with more moles of gas.