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LGS GCSE OCR Chemistry A > C5 Monitoring and Controlling Chemical Reactions > Flashcards

C5 Monitoring and Controlling Chemical Reactions Flashcards

1
Q

What is atom economy

A

The atom economy is a measure of how many atoms in the products make up the desired product.

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2
Q

What is the formula used to calculate atom economy

A

π΄π‘‘π‘œπ‘š π‘’π‘π‘œπ‘›π‘œπ‘šπ‘¦= (Sum of π‘€π‘Ÿ π‘œπ‘“ π‘‘π‘’π‘ π‘–π‘Ÿπ‘’π‘‘ π‘π‘Ÿπ‘œπ‘‘π‘’π‘π‘‘/Sum of π‘€π‘Ÿ π‘œπ‘“ π‘Žπ‘™π‘™ π‘π‘Ÿπ‘œπ‘‘π‘’π‘π‘‘s) x 100

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3
Q

What factors should be considered when making a substance?

A

Yield of the product
Atom economy
Usefulness of bi-products
Rate of reaction
Equilibrium position if reversible

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4
Q

What is Theoretical Yield

A

The theoretical yield is the maximum possible mass of desired products you can make from a given mass of reactants.

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5
Q

What is percentage yield

A

The percentage yield is the amount produced compared to your theoretical yield

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6
Q

How do you calculate percentage yield ?

A

π‘π‘’π‘Ÿπ‘π‘’π‘›π‘‘π‘Žπ‘”π‘’ 𝑦𝑖𝑒𝑙𝑑= (π‘Žπ‘π‘‘π‘’π‘Žπ‘™ yield) / (π‘‘β„Žπ‘’π‘œπ‘Ÿπ‘’π‘‘π‘–π‘π‘Žπ‘™ π‘šπ‘Žπ‘ π‘ ) π‘₯ 100

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7
Q

The equation for concentration

A

π‘ͺπ’π’π’„π’†π’π’•π’“π’‚π’•π’Šπ’π’= π‘¨π’Žπ’π’–π’π’•/π‘½π’π’π’–π’Žπ’†

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8
Q

Give units for concentration

A

g/dm3 or mol/dm3

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9
Q

What pieces of equipment are needed to carry out a titration

A

Burette, volumetric pipette, pipette filler, conical flask, white tile, clamp and stand, indicator.

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10
Q

What are concordant titre values

A

When the titre values are within 0.10 cm3

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11
Q

What is molar volume

A

1 mole of any substance in the gas state occupies the same volume at the same temperature and pressure
At room temperature and pressure (RTP) this volume is 24dm3 or 24000cm3

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12
Q

Write down the gas equations

A

π‘Žπ‘šπ‘œπ‘’π‘›π‘‘ (π‘šπ‘œπ‘™)= (π‘£π‘œπ‘™π‘’π‘šπ‘’ (π‘‘π‘š3))/24

π‘£π‘œπ‘™π‘’π‘šπ‘’ (π‘‘π‘š3 )=π‘Žπ‘šπ‘œπ‘’π‘›π‘‘ (π‘šπ‘œπ‘™) π‘₯ 24

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13
Q

What is rate of reaction

A

Measure of how quickly reactants are used or products are formed

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14
Q

Give formulae for measuring rate

A

π‘…π‘Žπ‘‘π‘’ π‘œπ‘“ π‘Ÿπ‘’π‘Žπ‘π‘‘π‘–π‘œπ‘›= (π΄π‘šπ‘œπ‘’π‘›π‘‘ π‘œπ‘“ π‘π‘Ÿπ‘œπ‘‘π‘’π‘π‘‘ π‘π‘Ÿπ‘œπ‘‘π‘’π‘π‘’π‘‘)/π‘‡π‘–π‘šπ‘’

π‘…π‘Žπ‘‘π‘’ π‘œπ‘“ π‘Ÿπ‘’π‘Žπ‘π‘‘π‘–π‘œπ‘›= (π΄π‘šπ‘œπ‘’π‘›π‘‘ π‘œπ‘“ π‘Ÿπ‘’π‘Žπ‘π‘‘π‘Žπ‘›π‘‘ 𝑒𝑠𝑒𝑑)/π‘‡π‘–π‘šπ‘’

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15
Q

What has to happen in order for a reaction to happen between 2 particles

A

The reacting particles need to collide
The collision needs to have enough energy (more than the activation energy) so that the particles will then react (bonds will break etc)

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16
Q

Predict what will happen in terms of collisions if we increase the temperature of a reaction

A

The number of collisions increase because the particles are moving more quickly.
The percentage of collisions which are successful increases because all the particles have more energy

17
Q

What is a catalyst?

A

A substance that increases the rate of the reaction but remains unchanged at the end.
They provide an alternative reaction pathway with a lower activation energy.

18
Q

What is a reversible reaction

A

A reversible reaction is one in which the products are able to react with each other to change back into the reactants without any additional changes

19
Q

Give an example of a reversible reaction

A

CuSO4.5H2O ↔ CuSO4 + 5H2O

20
Q

What is the equilibrium position

A

The position of equilibrium is related to the ratio of the concentration of products to the concentration of reactants

21
Q

State if true or false for the following:
At equilibrium reactants are still reacting to make products.
At equilibrium you always have equal amounts of reactants and products.
Equilibrium always happens at the same point no matter the conditions.
When you decrease the concentration of the reactants the equilibrium point will be closer to the left.
Equilibrium can only be reached in a closed system.

A

At equilibrium reactants are still reacting to make products TRUE
At equilibrium you always have equal amounts of reactants and products FALSE
Equilibrium always happens at the same point no matter the conditions FALSE
When you decrease the concentration of the reactants the equilibrium point will be closer to the left TRUE
Equilibrium can only be reached in a closed system TRUE

22
Q

What is Le Chatelier’s Principle?

A

Any change made to a reaction which is in equilibrium, will result in the equilibrium position moving to minimise the change made

23
Q

What factors might change the position of equilibrium?

A

Temperature
Concentration
Pressure

24
Q

What is dynamic equilibrium

A

The forward and backward reactions still happen and concentrations of all the reacting substances remain constant

LGS GCSE OCR Chemistry A (7 decks)

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