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Chemistry > Rates of Reaction / Reversible Reactions > Flashcards

Rates of Reaction / Reversible Reactions Flashcards

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1
Q

What is the rate of a reaction? - Rates of Reaction

A

A measure of how quickly a reactant is used up or how quickly a product is formed

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2
Q

What is collision theory? - Rates of Reaction

A

The theory that for a chemical reaction to happen reactant particles must collide with each other and the particles must have enough energy to react

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3
Q

What is a successful collision? - Rates of Reaction

A

A collision between reactant particles that has enough energy to create a reaction

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4
Q

What importance is activation energy for successful reactions? - Rates of Reaction

A

If particles do not have sufficient activation energy (the minimum amount of energy that colliding particles must have in order to react) a reaction won’t take place

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5
Q

What 2 ways can be used to calculate the mean rate of a reaction? What unit is used - Rates of Reaction

A

Rate of reaction = quantity of reactant used / time taken
OR quantity of product formed / time taken
Units in g/s or g/minute

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6
Q

How can the volume of gas produced in a reaction be measured? - Rates of Reaction

A

A gas syringe can be placed in a bung on a conical flask and it will measure the volume of gas produced

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7
Q

How can the gradient of a rate of reaction graph be useful to us? - Rates of Reaction

A

The gradient of the line shows the rate of reaction (steep gradient = quick reaction)

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8
Q

How does the concentration of reactants affect the rate of reaction? - Rates of Reaction

A

The reactant particles become more crowded as there are more of them, which increases the frequency of successful collisions and increases the rate of a reaction

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9
Q

How does the pressure of reactants (gas) affect the rate of reaction? - Rates of Reaction

A

By increasing the pressure, reactant particles become more crowded, increasing the frequency of successful collisions, and increasing the rate of reaction

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10
Q

How can you calculate the rate of a reaction at a given stage of the reaction? - Rates of Reaction

A

By drawing a tangent to the curve on the graph, calculate the gradient of this tangent to find the rate of the reaction

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11
Q

How does surface area : volume ratio affect the rate of a reaction? - Rates of Reaction

A

The higher the surface area to volume ratio, more reactant particles are exposed at the surface. This means that the frequency of successful collisions between reactants increases, increasing the rate of reaction

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12
Q

How does temperature affect the rate of a reaction? - Rates of Reaction

A

It increases the internal (kinetic) energy of the particles, meaning more particles have activation energy, meaning the number of successful collisions increases. Rate increases.

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13
Q

What is a catalyst? - Rates of Reaction

A

A substance that increases the rate of a chemical reaction without being used up

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14
Q

How do catalysts work? - Rates of Reaction

A

Provides an alternative reaction pathway with a lower activation energy. Increases the frequency of successful collisions

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15
Q

How do a catalysts effects appear on a reaction profile? - Rates of Reaction

A

The activation energy is lower than previously, therefore the gradient of the loop on the graph is smaller

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16
Q

What is a reversible reaction? - Reversible Reactions

A

A reaction where the reactants can be converted into products and products back into reactants

17
Q

What rule is there for reversible reactions regarding endothermic and exothermic reactions? - Reversible Reactions

A

If a reaction is endothermic one direction, then it is exothermic in the other

18
Q

Which direction is the equilibrium of a forward and backward reaction? - Reversible Reactions

A

The forward reaction goes to the right

The backward reaction goes to the left

19
Q

How does a reversible reaction work in terms of hydrated copper sulfate? - Reversible Reactions

A

As the hydrated copper sulfate is heated, the water molecules are driven off, leaving ANHYDROUS copper sulfate. By adding water, the copper sulfate becomes hydrated again

20
Q

What is an equilibrium? - Reversible Reactions

A

A state where the forward and backward reactions are happening at the same rate, with the concentrations of all reactants being constant

21
Q

What is dynamic equilibrium? - Reversible Reactions

A

A state of balance between continuing processes

22
Q

Describe the Haber process - Reversible Reactions

A

Nitrogen gas is reacted with hydrogen gas to make ammonia gas. The forward reaction is exothermic

23
Q

What is Le Chatelier’s principle? - Reversible Reactions

A

The idea that if the conditions of a reversible reaction are altered, the equilibrium will shift to oppose the change

24
Q

How can the reaction conditions be changed in a reversible reaction? - Reversible Reactions

A

Changing the PRESSURE
Changing the CONCENTRATION
Changing the TEMPERATURE

25
Q

When a change is made to a system at equilibrium, what does the equilibrium do? - Reversible Reactions

A

The equilibrium position changes to oppose the change made

26
Q

Name an example of the equilibrium opposing a change - Reversible Reactions

A

If the temperature of a reaction is increased, the position of the equilibrium will shift to the endothermic direction to reduce the temperature

27
Q

If pressure is increased in a reaction involving gases, what happens to the equilibrium? - Reversible Reactions

A

The equilibrium will shift in the direction of the fewest molecules of gas to reduce the pressure, producing more of the product with fewer molecules

28
Q

What is the formula equation for the Haber process? - Reversible Reactions

A

N2 (g) + 3H2 (g) <=> 2NH3 (g)

29
Q

What does the equilibrium do if the temperature of a reaction increases? - Reversible Reactions

A

The equilibrium shifts to the endothermic side, producing more of the product in an endothermic reaction

30
Q

If the forward reaction in the Haber process (producing ammonia) is exothermic and the temperature increases, what happens? - Reversible Reactions

A

The equilibrium will shift to the endothermic side (producing Nitrogen and Hydrogen) to reduce the temperature and produce more nitrogen and hydrogen

31
Q

What happens if a concentration of a reactant is increased in a reversible reaction? - Reversible Reactions

A

The equilibrium will shift to the side with fewer reactants to produce more of the reactants with a smaller concentration

32
Q

What happens when metals react with dilute acids?

A

Form a Metal salt and hydrogen

33
Q

What do alkalis react with acids to form?

A

Salt and water

Chemistry (11 decks)

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