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Edexcel GCSE Chemistry > Topic 5a Mass calculations, electrolysis, extraction of metals and equilibria > Flashcards

Topic 5a Mass calculations, electrolysis, extraction of metals and equilibria Flashcards

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1
Q
  1. What is the formula of water?
A

H2O

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2
Q
  1. What is the formula of sodium chloride?
A

NaCl

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3
Q
  1. What is the formula of carbon dioxide?
A

CO2

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4
Q
  1. The formula of magnesium chloride is MgCl2. What is the ratio of magnesium ions to chloride ions?
A

1:2

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5
Q
  1. The formula of sulfuric acid is H2SO4. How many atoms of each element are in the formula?
A

H = 2, S = 1, O = 4

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6
Q
  1. The formula of calcium nitrate is Ca(NO3)2. How many calcium, nitrogen and oxygen atoms are in the formula?
A

Ca = 1, N = 2, O = 6

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7
Q
  1. There are two numbers alongside chlorine in the periodic table, 17 and 35.5. What does the number 17 represent?
A

atomic number

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8
Q
  1. What does the number 35.5 represent?
A

relative atomic mass

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9
Q
  1. Sodium chloride has the formula NaCl. The relative atomic mass of sodium is 23 and that of chlorine is 35.5. What is the relative formula mass of NaCl?
A

58.5

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10
Q
  1. A water molecule has the formula H2O. The relative atomic mass of hydrogen is 1 and that of oxygen is 16. What is the relative formula mass of a molecule of water?
A

18

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11
Q
  1. What is the symbol for relative atomic mass?
A

Ar or RAM

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12
Q
  1. What is the symbol for relative formula mass?
A

Mr or RFM

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13
Q
  1. The relative atomic mass of hydrogen is 1. What is the relative formula mass of hydrogen molecules?
A

2

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14
Q
  1. Sodium chloride has the formula NaCl; the relative atomic mass of sodium is 23 and that of chlorine is 35.5. What is the relative formula mass of NaCl?
A

58.5

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15
Q
  1. A water molecule has the formula H2O; the relative atomic mass of hydrogen is 1 and that of oxygen is 16. What is the relative formula mass of water?
A

18

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16
Q
  1. A carbon dioxide molecule has the formula CO2; the relative atomic mass of carbon is 12 and that of oxygen is 16. What is the relative formula mass of carbon dioxide?
A

44

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17
Q
  1. What is the empirical formula of a compound with molecular formula C2H4?
A

CH2

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18
Q
  1. What is the empirical formula of a compound with molecular formula C3H8?
A

C3H8

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19
Q
  1. A sample of magnesium carbonate was heated in an open test tube. Why did it lose mass?
A

gas/carbon dioxide escaped

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20
Q
  1. 100 cm3 of a solution contained 2 g of salt. What is the concentration of the salt in g dm-3?
A

20

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21
Q
  1. A sample of copper carbonate was heated in an open test tube. Why did it lose mass?
A

gas/carbon dioxide escaped

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22
Q
  1. Why does magnesium increase in mass when it is heated in air?
A

combines with oxygen

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23
Q
  1. How many cm3 are there in 1 dm3?
A

1000

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24
Q
  1. What is 250 cm3 expressed in dm3?
A

0.25

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25
Q
  1. What is 0.5 dm3 expressed in cm3?
A

500

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26
Q
  1. 100 cm3 of a solution contains 1.5 g of salt. What is the concentration of the salt solution in g dm3?
A

15

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27
Q
  1. 250 cm3 of a solution contains 5 g of sugar. What is the concentration of the sugar solution in g dm3?
A

20

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28
Q
  1. A solution of copper sulfate has concentration 10 g dm3. What mass of copper sulfate will be dissolved in 100 cm3 of solution?
A

1 g

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29
Q
  1. 2 g of hydrogen reacts with oxygen to form 18 g of water. What mass of water will be formed from 1 g of hydrogen?
A

9 g

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30
Q
  1. 2H2 + O2 → 2H2O. How many molecules of hydrogen are needed to react with 1 dozen molecules of oxygen to form water?
A

2 dozen

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31
Q
  1. What is the abbreviation used for the mole, the unit for amount of substance?
A

mol

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32
Q
  1. How many particles are there in 1 mole of particles?
A

6.02 x 1023

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33
Q
  1. The mass of 1 mole of carbon atoms is 12 g. What is the mass of 2 moles of carbon atoms?
A

24 g

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34
Q
  1. What is the formula for calculating the number of moles of substance from its mass in g
A

moles = mass (g) / RAM or RFM

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35
Q
  1. Each water molecule contains three atoms. How many moles of atoms are there in 2 moles of water molecules?
A

6 mol

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36
Q
  1. The relative formula mass of chlorine gas is 71. What is the mass of 1 mole of chlorine gas?
A

71 g

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37
Q
  1. What is the Avogadro number?
A

6.02 x 1023 the number of atoms/particles in a mole

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38
Q
  1. What is the emperical formula of a compound?
A

The simplist whole number ratio of atoms in compound

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39
Q
  1. What is the law of conservation of mass?
A

total mass of reactants = total mass of products

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40
Q
  1. How are the emperical formula and molecular formula related?
A

The molecular formula is a multiple of the emperical formula

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41
Q
  1. What name is given to an atom that has gained or lost electrons?
A

ion

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42
Q
  1. What type of charge is on metal and hydrogen ions?
A

positive

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43
Q
  1. What type of charge is on most non-metal ions?
A

negative

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44
Q
  1. What is another name for a positive ion?
A

cation

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45
Q
  1. What is another name for a negative ion?
A

anion

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46
Q
  1. What is the symbol for a sodium ion?
A

Na+

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47
Q
  1. What is the symbol for a magnesium ion?
A

Mg2+

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48
Q
  1. What is the symbol for a chloride ion?
A

Cl<span>-</span>

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49
Q
  1. What is the symbol for a sulfate ion?
A

SO42-

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50
Q
  1. In what states do ionic compounds conduct electricity?
A

when molten or dissolved in water

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51
Q
  1. Which of these is not an electrolyte: solid sodium chloride, molten sodium chloride, aqueous sodium chloride?
A

solid sodium chloride

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52
Q
  1. What is the name of the positively charged electrode?
A

anode

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53
Q
  1. What type of ions are attracted to the positively charged electrode?
A

anions / negative ions

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54
Q
  1. What is the name of the negatively charged electrode?
A

cathode

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55
Q
  1. What type of ions are attracted to the negatively charged electrode?
A

cations / positive ions

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56
Q
  1. H What process takes place when a substance gains electrons?
A

reduction

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57
Q
  1. H In terms of subatomic particles, what happens to a substance when it is oxidised?
A

It loses electrons.

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58
Q
  1. H What type of reaction takes place at the anode during electrolysis?
A

oxidation

59
Q
  1. What are inert electrodes made from?
A

graphite / platinum

60
Q
  1. What is produced at the cathode when molten lead bromide is electrolysed?
A

lead

61
Q
  1. What gas is formed when sodium reacts with water?
A

hydrogen

62
Q
  1. What solution is formed when sodium reacts with water?
A

sodium hydroxide

63
Q
  1. What colour is universal indicator when added to sodium hydroxide?
A

blue or purple

64
Q
  1. What gas is formed when magnesium is added to dilute sulfuric acid?
A

hydrogen (MASH)

65
Q
  1. What solution is formed when magnesium reacts with dilute sulfuric acid?
A

magnesium sulfate

66
Q
  1. What would you see when magnesium is added to dilute sulfuric acid?
A

effervescence/fizzing/bubbles/magnesium disappears

67
Q
  1. Name a metal that does not react with water or dilute acids.
A

copper/silver/gold/platinum

68
Q
  1. What products are formed when zinc is added to copper sulfate solution?
A

zinc sulfate and copper

69
Q
  1. What type of reaction takes place when zinc is added to copper sulfate solution?
A

displacement

70
Q
  1. Magnesium reacts with chromium nitrate solution to form magnesium nitrate and chromium. Which metal is more reactive?
A

magnesium

71
Q
  1. Name a metal that reacts vigorously with cold water.
A

potassium/sodium/rubidium/caesium/lithium/calcium

72
Q
  1. What gas is produced when a metal reacts with water?
A

hydrogen

73
Q
  1. How do you test for the hydrogen gas?
A

It pops a lighted splint.

74
Q
  1. What type of solution is formed when a metal reacts with water - acidic, alkaline or neutral?
A

alkaline

75
Q
  1. What salt is formed when zinc reacts with hydrochloric acid?
A

zinc chloride

76
Q
  1. Complete the word equation, magnesium + copper sulfate makes …
A

copper + magnesium sulfate

77
Q
  1. What type of ions are formed from metal atoms when they react with acids?
A

cations/positive ions

78
Q
  1. What type of reaction takes place when a substance loses oxygen?
A

reduction

79
Q
  1. Name a metal that occurs uncombined in the Earths crust.
A

gold/silver/platinum

80
Q
  1. Name a metal that could be extracted from its metal oxide by heating with carbon.
A

zinc/iron/copper

81
Q
  1. Name a metal that occurs uncombined in the Earths crust.
A

gold/silver/platinum

82
Q
  1. Name a metal, other than iron, that could be extracted from its metal oxide by heating with carbon.
A

zinc/copper

83
Q
  1. What compound of carbon is formed when it is heated with copper oxide?
A

carbon dioxide/carbon monoxide

84
Q
  1. Why is electrolysis not used to extract iron from iron oxide?
A

too expensive/too much energy needed

85
Q
  1. Why is aluminium not extracted by heating aluminium oxide with carbon?
A

aluminium is more reactive than carbon/carbon is not reactive enough to remove the oxygen

86
Q
  1. What is the aluminium oxide dissolved in to form the electrolyte for electrolysis?
A

molten cryolite

87
Q
  1. What are the electrodes made from?
A

carbon/graphite

88
Q
  1. At which electrode is the aluminium produced?
A

cathode/negative electrode

89
Q
  1. What type of reaction takes place when a metal is extracted from its ore?
A

reduction/redox

90
Q
  1. What type of reaction takes place when a metal corrodes?
A

oxidation/redox

91
Q
  1. What is the definition of oxidation, in terms of oxygen?
A

gain of oxygen

92
Q
  1. H What is the definition of oxidation, in terms of electrons?
A

loss of electrons

93
Q
  1. What type of reaction takes place when metals are extracted from their ores?
A

reduction/redox

94
Q
  1. What is the specific name for the corrosion of iron?
A

rusting

95
Q
  1. Which of these metals will corrode most quickly - iron, sodium, copper?
A

sodium

96
Q
  1. Why does sodium corrode most quickly.
A

most reactive metal corrodes most quickly

97
Q
  1. Which substance has been oxidised in this reaction - copper oxide + hydrogen → copper + water?
A

hydrogen

98
Q
  1. Which substance has been reduced in in this reaction - copper oxide + hydrogen → copper + water?
A

copper oxide

99
Q
  1. What name is given to a process that converts an unwanted product into a new, useful product?
A

recycling

100
Q
  1. Name a type of substance that can be recycled.
A

metal, plastic, paper, cardboard, glass, etc.

101
Q
  1. What can happen in a reversible reaction?
A

the products can reform the reactants

102
Q
  1. What does the term equilibrium describe?
A

a position of balance

103
Q
  1. What is the process used to make ammonia?
A

Haber Process

104
Q
  1. What is the molecular formula of ammonia?
A

NH3

105
Q
  1. What is the balanced symbol equation for making ammonia from Nitrogen (N2) and Hydrogen (H2)
A

N2 +3H2 → 2NH3

106
Q
  1. Where does nitrogen come from for use in the Haber Process?
A

From the fractional distillation of air

107
Q
  1. Where does Hydrogen come from for use in the Haber process?
A

From methane from crude oil

108
Q
  1. What conditions of pressure are required to increase the yield of ammonia in the Haber Process?
A

High pressure (because there are more molecules on the LHS of the equation)

109
Q
  1. The forward reaction is exothermic. What conditions of temperature are required to increase the yield of ammonia in the Haber Process?
A

Low temperature (The equilibrium will shit to try and produce heat)

110
Q
  1. Theoretically, a high yield of ammonia is produce at low temperature and high pressure. Why is this not used in reality?
A

Low temperatue will result in a slow rate of reaction. High pressures are expensive and dangerous.

111
Q
  1. It was found that metal X didn’t react with dilute acids. What does this definitely tell us about the position of Metal X in the reactivity series?
A

It is below hydrogen in the reactivity series. This is because metals above hydrogen can displace hydrogen from dilute acids.

112
Q
  1. What happens at the positive anode always?
A

Oxidation

113
Q
  1. What happens at the negative cathode always?
A

Reduction

114
Q
  1. Most metals can be extracted from their ores by electrolysis. What is the main reason that copper metal isn’t extracted from its ore by electrolysis?
A

The main reason that copper metal isn’t extracted from its ore by electrolysis is that the process uses a lot of electrical energy. Many extraction methods produce unwanted waste gases anyways.

115
Q
  1. What factor does the biological extraction of copper, using phytoextraction, depend on?
A

That plants can take in copper compounds from the soil

Phytoextraction concentrates the copper in the plant, which is collected and burned. The metal can be obtained from the ash.

116
Q
  1. When a metal is extracted from its ore using carbon, what is oxidised?
A

The carbon is oxidised as it gains oxygen.

The metal oxide is reduced.

117
Q
  1. What products are formed when zinc metal reacts with steam?
A

Metal + steam → metal oxide + hydrogen.

Hydroxides are formed in the reactions of metals with liquid water.

118
Q
  1. What conditions of temperature and pressure are used in the industrial manufacture of ammonia?
A

temperature = 450 °C

pressure = 200 atmospheres.

119
Q

119.

One of the stages in sulfuric acid production is described by this equation:

2SO2(g) + O2(g) ⇌ 2SO3(g).

What will happen to the yield of SO3 if the pressure is increased?

A

If the pressure is increased, the SO3 yield will go up as the equilibrium position moves in the direction which forms less molecules of gas.

120
Q
  1. If the forward reaction in a reversible reaction is endothermic, what will be the effect of decreasing the temperature?
A

The effect of decreasing the temperature would be to decrease the amount of products at equilibrium as the equilibrium position moves in the backward direction which is exothermic.

121
Q

121.

What is the effect of decreasing the pressure on the following equilibrium:

2NO(g) + O2(g) ⇌ 2NO2(g)?

A

The effect of increasing the pressure is to produce less NO2, as the equilibrium shifts in the direction which produces more gas molecules.

122
Q
  1. What effect on the equilibrium position is produced by adding a catalyst to a system in equilibrium? - Higher
A

Adding a catalyst has no effect on the position of equilibrium so the yield of products is unchanged.

123
Q
  1. When is an equilibria acheived in a closed or open system?
A

Closed so none of the products or reactants can escape.

124
Q
  1. What is an electrolyte?
A

An ionic compound either dissolved in solution or molten

125
Q
  1. What is an electrode?
A

The material used to supply electricity to the electrolyte (usually carbon or platinum)

126
Q
  1. In the elctrolysis of copper sulphate, the electrodes are made of copper. Which decreases and increases in weight?
A

The anode decreases in weight.

The cathode increases in weight.

Copper is transferred from the anode to the cathode.

127
Q

What are the equations at the electrodes in the elctrolysis of copper sulphate using copper electrodes?

A

Equations at electrodes (HIGHER)

At the Cathode

Cu2+ + 2e- → Cu This is Reduction

At the Anode

Cu - 2e- → Cu2+ This is Oxidation

128
Q
  1. What are the rules for what is produced in electrolysis?
A

Rules for competition at electrodes

At the cathode – the least reactive metal will win

At the anode – the least complex ion will win

Halide > Hydroxide > all other negative ions

129
Q
  1. What is the order of the reactivity series?
A
130
Q

In the electrolysis of copper sulphate using INERT ELECTRODES, What is formed at the anode and cathode? And why?

A

Ions present : Cu2+ , H+ , OH- , SO42-

At the cathode (Copper) Cu2+ + 2e- → Cu Red.

At the anode (Oxygen) 4OH– – 4e– → O2 + 2H2O Ox.

Because

Copper is less reactive than hydrogen so is formed

OH- is a more simple ion than SO42- so oxygen is formed

131
Q
  1. What are the metals you can and can’t extrct from their ores.
A
132
Q
  1. How can you extract copper from it’s ore?
A

heating (smelting)

Bio leaching

Phytomining

133
Q

What is bio leaching?

A

Uses bacteria to concentrate the copper called a leachate.

copper is extracted from the lechate by displacement using scrap ion, then purified by electrolysis.

134
Q

What is Phytoextraction/ Phytomining?

A

Uses plants to concentrate the copper. The plants absorb the metal compounds then the plants are burnt to form ash, from which the metal is extracted.

135
Q

What are the advantages and disvantages of bioleaching?

A

does not require high temperatures

toxic substances and sulphuric acid can be produced by the process, and damage the environment.

136
Q

What are the pros and cons of phytoextraction/mining?

A

can extract metals from contaminated soils

more expensive than mining some ores. growing plants is dependent on weather conditions.

137
Q

Pros and cons of using both bio leaching and pytoextraction/mining?

A

no harmful gases are produced.

causes less damage to the landscape than mining.

conserves supplies of higher garde ores.

very slow process.

138
Q

When extracting aluminium or metals using electrlysis what is produced at the cathode and anode?

A

Ions present : Al3+ , O2-

At the cathode (Aluminium)

Al3+ + 3e- → Al

At the anode (Oxygen)

2O2– – 4e– → O2

139
Q

What is the balanced making ammonia The haber process equation?

A

N2 (g) + 3H2 (g) 2NH3 (g) + Heat

140
Q

What three factors effect the posistion of the equilibrium?

A

(not catalysts they only speed up the process)

temperature

pressure

concentration?

141
Q

What are the effects of concentration, pressure and temperature on the position of an equilibrium.

A

1 concentration

If the concentration of reactant is increased more products are made to use them up.

If the concentration of products are decreased more products will be made to replace them.

2 pressure

If the pressure is increased the equilibrium will shift to the side of the reaction with less molecules of gas to try to reduce the pressure.

3 temperature

If the temperature is decreased the equilibrium will shift to the side that produces heat to try to heat it up.

142
Q

what is the catalyst used in the haber process?

A

Iron catalyst.

143
Q
A

Edexcel GCSE Chemistry (13 decks)

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