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G10 > G10 CHEM > Flashcards

G10 CHEM Flashcards

1
Q

Reversible reactions

A

Both forward and the reverse reaction can occur as the product molecules can themselves react with each other or decompose and form the reactant molecules again

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2
Q

If the forward reaction is exothermic, the reverse will be

A

endothermic as the same amount of heat is transferred in both direction

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3
Q

Equilibirum

A

A system is said to be in equilibrium when the rate of forward reaction is equal to the rate of the backward reaction and the concentration of reactant and product becomes constant in a reversible reaction in a close system

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4
Q

More product than reactant,

A

Equilibrium lies to the right

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5
Q

More reactant than product

A

Equilibrium lies to the products side

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6
Q

Types of equilibrium

A

Physical and Chemical

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7
Q

Physical equilibrium

A

If there is a physical change and only the state changes

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8
Q

Chemical equilibrium

A

If there is a chemical change and new substance is formed

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9
Q

Example of physical equilibrium reaction

A

Any hydrated salt breaking down into anhydrous salt + water

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10
Q

Le chatelier’s principle

A

When a system in equilibrium is disturbed, the equilibrium wants to undo the disturbance to go back to equilibrium

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11
Q

What are the factors affecting equilibrium

A

Temp
Pressure
Concentration
Catalyst

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12
Q

How does a change in temperature affect the equilibrium

A

Increasing the temperature shifts the equilibrium to endothermic side

Decreasing the temperature shifts the equilibrium to the exothermic side

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13
Q

How does a change in the pressure affect the equilibrium

A

Increase in pressure means no of particles per unit volume increase and hence equilibrium wants to go to side with less particles. Decreasing the pressure means the equilibrium will shift to the side with more gas molecules. This is because reducing the pressure makes the system want to occupy more volume

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14
Q

3H_2 + N_2 ⇌ 2NH_3

where will the equilibrium shift

A

3 + 1 = 4 > 2

Hence equilibrium will shift in forward direction, increasing the yield of ammonia

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15
Q

How does a change in the concentration affect the equilibrium

A

Increasing the concentration of reactants/Decreasing concentration of products = equilibrium shifts in forward direction

Increasing concentration of products/Decreasing concentration of reactant = equilibrium shifts in reverse direction

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16
Q

How does adding a catalyst affect the equilibrium

A

Add a catalyst = increase rate of forward reaction and backward reaction in the same manor

Adding catalyst means equilibrium will be achieved faster, but they will have no effect in the yield of products/reactants

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17
Q

In an equilibrium graph, what happens to the lines of rate of forward and reverse reaction

A

The line representing rate of forward reaction gradually decreases before becoming constant

The line representing rate of reverse reaction gradually increase before becoming constant

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18
Q

What is the region called where the rate of forward and backward reactions are not constant, ie the region before equilibrium

A

Kinetic region

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19
Q

Haber’s process

A

industrial method for ,making ammonia (NH₃) from nitrogen (N₂) and hydrogen (H₂) gases at high pressure, moderate temperature and with a catalyst

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20
Q

Why is Haber process important in daily life

A

Haber process makes ammonia, which is an essential ingredient in the production of fertilisers, which helps grow the crops we eat

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21
Q

Redox Reaction

A

A reaction where oxidation and reduction both happen simultaneously

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22
Q

Conditions for oxidation to happen

A

1) gain of oxygen
2) Loss of electrons
3) Loss of hydrogen atoms
4) Increase in oxidation number

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23
Q

conditions for reduction to happen

A

1) loss of oxygen
2) gain of electrons
3) gain of hydrogen atoms
4) decrease in oxidation number

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24
Q

Who will undergo oxidation or reduction

A

Only reactants

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25
Q

Reactant which oxidises

A

Reductant/Reducing agent

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26
Q

Reactant which is reduces

A

Oxidizing Agent/Oxidant

27
Q

4 main properties to remember to convert molecular equations into ionic equations

A

Solids, liquid and gases cant disassociate into ions

only aqueous solutions will disassociate

Solids always lose electrons

Aqueous will always gain electrons

28
Q

atoms in free state oxidation no

A

0

29
Q

oxidation number of group 1 elements in all its compounds

A

+1

30
Q

oxidation number of group 2 elements in all its compounds

A

+2

31
Q

oxidation number of oxygen in all its compounds

A

-2

32
Q

oxidation number of group 7/17 elements in all its compounds

A

-1

33
Q

oxidation number of hydrogen in all its compounds

A

+1

34
Q

Oxidation number of monoatomic ions

A

change present on the ions

35
Q

Sum of oxdiation numbers in a compounds is equal to

A

0

36
Q

Sum of oxidation number in a polyatomic ion is equal to

A

charge present on ion

37
Q

what happens in rusting and corrosion in terms of redox reactions

A

metal is oxidized (loses electrons), and typically oxygen is reduced (gains electrons)

38
Q

All nitrates and sulphates are…

A

soluble in water

39
Q

colour of copper salt

A

blue, shade depends on centration of salt of copper present

40
Q

Reactivity series of metals pneumonic

A

Katrina Ne Car Maangi Alto Zen Ferrari Tesla, PhirBhi [Haye] Cyu Mili Silver Audi Plated

41
Q

Reactivity series of metal actual

A

K - Potassium
Na - Sodium
Ca - Calcium
Mg - Magnesium
Al - Aluminium
Zn - Zinc
Fe - Iron
Sn - Tin
Pb - Lead
[H] - hydrogen
Cu - Copper
Hg - Mercury
Ag - Silver
Au - Gold
Pt - Platinium

42
Q

What is electrolysis

A

On passing electric current in a molten or aqueous solution a chemical reaction takes place in an ionic compound an it disassociates into its elements.

43
Q

Electrodes

A

Electrical conductors (metals) which allow for the flow of charge to pass

44
Q

Active Electrodes

A

Interfere with electrolysis reaction. They are mainly metals with low reactivity

45
Q

Inert electrodes

A

Dont interfere in electrolysis reaction. Mainly graphite of platinum

46
Q

Electrolytic cell

A

Any appartus used in electrolysis

47
Q

Electrolyte

A

Ionic compound in liquid/molten/aqueous state

48
Q

Cathode

A

Negatively charged electrode (always connected to negative terminal of battery)
Attracts cations in compound
Reduction takes place at cathode due to gain of electrons

49
Q

Anode

A

Positively charged cathode (always connected to positive terminal of battery)
Attract anions in compound
Oxidation takes place due to loss of electrons

50
Q

When current flows in electrolyte vs when current flows in electrode +wires who carry the charge

A

Electrolyte =Ions
Electrode + Wires = electrons

51
Q

Does cathode attract more reactive or less reactive metals

A

Less reactive

52
Q

Anode formula for electrolysis for OH^-1

A

4OH^-1 = O_2 + 2H_2O + 4e^-1

53
Q

Which ions and elements move to cathode

A

Hydrogen and Metal Ions

54
Q

Factors affecting deposition in Electrolysis using Active electrode

A

Time
Voltage/Potential Difference
Concentration

55
Q

What all changes can be seen when an inert electrode is used

A

Colour of electrolyte fades as ions are leaving the solution
No change in mass of Anode
Cathode mass increase as a layer of solid is being deposited on the cathode.

56
Q

What all changes can be seen when an active electrode is used

A

colour of electrolyte remains the same as ions keep flowing back in the solution
Anode mass decreases
Cathode mass increase

57
Q

How does increasing the concentration affect the rate of deposition

A

Increasing the concentration means more ions are present in the electrolyte and hence a greater number of ions will be attracted to the cathode forming a greater deposition layer

58
Q

How does increasing the potential difference affect the rate of deposition

A

Higher voltage leads to more movement of ions in the electrolyte, resulting in a greater number of metal ions being deposited on the cathode. According to Ohm’s Law, a greater voltage supplied means a greater current flowing through the electrolyte. Increased current enhances the rate at which metal ions are reduced and deposited on the cathode, with more ions moving towards the cathode per unit time

59
Q

How does increasing the time affect the rate of deposition

A

Increasing the time means a longer duration for the ions to deposit onto the cathode, hence a greater rate of deposition

60
Q

What interference will the active electrodes have on electrolysis

A

At Anode, the deposition of anions will happen, however, the electrons present in element of anode will also be pulled by the battery and hence the the newly formed ions from the anode will deposit into the electrolyte, refilling the hole leaved by the cation present in the electrolyte being attached to the cathode

61
Q

Electroplating material of anode and electrolyte

A

Must be the material or contain the material you wish to electroplate on cathode. Metal in electrolyte must be same as Anode

62
Q

The object you want to electroplate must be the

A

Cathode

63
Q

Salt Bridge

A

Helps maintain neutrality of solution and helps in movement of ions (cations move to cathode and anion move to anode)

Use metal of high reactivity to ensure no interference in reaction

64
Q

Factors affecting Voltage in Voltaic Cell

A

Electrode Material - Different materials have different tendencies to lose or gain electrons
Electrolyte concentration - Increasing the electrolyte concentration in a voltaic cell increases the voltage by enhancing the availability of ions for the reaction
Surface Area of electrode - A larger surface area allows for more contact between the electrode and electrolyte hence a greater voltage
Temperature - Higher temperature means a higher resistance making it harder for current to flow

G10 (5 decks)

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