C6 Flashcards

1
Q

What is the mean rate of reaction equation?

A

Quantity of reactant used / time taken OR Quantity of product produced / time taken

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2
Q

What can the quantity of a reactant or product be measured in?

A

Mass in grams or by a volume in cm^3

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3
Q

What is the unit for rate of reaction?

A

g/s cm3/s

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4
Q

What are some factors which affect the rates of chemical reaction? (5)

A
  1. Concentrations of reactants. / Pressure in gases 2. Surface area of solid reactants 3. Temperature 4. Presence of catalysts
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5
Q

How does increasing the temperature increase the rate of reaction?

A

The particles all move faster. They are going to successfully collide. ore frequently. When they move faster, they have more energy which is needed for the reaction to happen.

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6
Q

How does increasing the concentration or pressure of gases increase the rate of reaction?

A

I

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7
Q

How does increasing the pressure of gases (reactants) increase the rate of reaction?

A

There are the same number of particles in a smaller space. So the successful collisions are more frequent.

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8
Q

How does increasing the surface area increase the rate of reaction?

A

Particles have more area (exposed particles) to collide with = more frequent collisions

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9
Q

How does using a catalyst increase the rate of reaction?

A

It speeds up the reaction without being used up in the reaction itself. They usually decrease the activation energy needed by finding an alternative path.

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10
Q

Required practical 5 - Magnesium + HCl reaction to produce H2 gas

A
  1. Add dilute HCl to a conical flask and measure it on a mass balance. 2. Add Magnesium ribbon to acid and plug with cotton wool. 3. Start the stopwatch and record the mass at regular intervals. 4. Plot the results in a table and work out mass loss. 5. Repeat with more concentrated acids. It should show higher concentration gives a faster rate of reaction.
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11
Q

Required practical 5 - sodium thiosulfate and HCl to produce cloudy precipitate.

A
  1. Add dilute sodium thiosulfate to a conical flask. 2 Place a piece of paper with a black cross on it. Add HCl and start stopwatch. 3. Watch cross disappear. 4. Reaction can be repeated with reactants of different concentrations. Higher concentration means quicker reaction.
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12
Q

What does the collision theory say?

A

Collision theory says that chemical reactions can only occur when reacting particles collide with each other and have sufficient energy.

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13
Q

What is the activation energy?

A

Energy which particles must need to start a reaction.

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14
Q

What does increasing the concentration; pressure and surface area do to the particles?

A

They collide more frequently so increases the rate of reaction.

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15
Q

What does increasing the temperature do to the particles?

A

Increases the frequency of the particles and makes the particles more energetic so increases the rate of reaction.

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16
Q

How does a graph with a catalyst compared to a graph without?

A

The activation energy is lower on the graph with the catalyst.

17
Q

How is a reversible reaction represented? (equation)

A

A +B ⇌ C + D

18
Q

Give an example of how reversible reactions can be changed by changing the conditions.

A

When you heat ammonium chloride —> ammonia + hydrogen chloride. When you let ammonia + hydrogen cool —> ammonium chloride.

19
Q

If a reversible reaction is exothermic one way; what is it the other way?

A

Endothermic

20
Q

What occurs when a reversible reaction occurs in a closed system?

A

Equilibrium is reached when both reactions occur at the same rate.

21
Q

What is Le Chantelier’s Principle?

A

If you change the conditions of a reversible reaction at equilibrium, the system will try to counteract that change.

22
Q

According to Le Chantelier’s Principle; what reaction is favoured if the temperature decreases?

A

The exothermic reaction would be favoured so more heat is given to warm up the surroundings. More products from the exothermic reaction will be made.

23
Q

According to Le Chantelier’s Principle; what reaction is favoured if you increase the pressure?

A

It favours the side with the least moles.

24
Q

According to Le Chantelier’s Principle; what happens when you increase the concentration of the reactants?

A

The amount of products increase.

25
Q

According to Le Chantelier’s Principle; what happens when you increase the concentration of the products?

A

The amount of reactants increase.