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GRADE 10
PHYSICAL SCIENCE
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1.
Aluminium𝑨𝒍
phosphorus
carbon dioxide
Hydrogen sulfate
Hydrochloric acid
Sulfuric acid
𝑷
𝑪𝑶𝟐
𝑯𝟐𝑺𝑶𝟒
𝑯𝑪𝒍
𝑯𝟐𝑺𝑶𝟒
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2.
Gaseous state (g)Liquid state (l)Solid state (s)Aqueous solution (aq)
𝑁2(𝑔) + 2𝑂2(𝑔) → 2𝑁𝑂2(𝑔)
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3.
𝑁2(𝑔) + 2𝑂2(𝑔) → 2𝑁𝑂2(𝑔)
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4.
𝑁2(𝑔) + 2𝑂2(𝑔) → 2𝑁𝑂2(𝑔)
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2(𝑁𝐻4)2𝐶𝑂3
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Examples• Write a balanced chemical equation for the following chemical reactions:
•Aluminium reacts with hydrogen chloride solution to form an aluminium chloride solution and hydrogen gas.
•Nitrogen gas reacts with hydrogen gas to form nitrogen hydride gas (ammonia gas)
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Homework
EXERCISE 14 PG. 158-159
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Energy changes
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• Energy changes in chemical reactions are bigger than the energy changes in physical changes.
•During a chemical change, the temperature increases or decreases because the kinetic energy of the
particles change.
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REMEMBERWhen bonds are broken – energy is absorbed
When new bonds are formed – energy is released
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Calculating energy change
• Amount of potential energy absorbed to break the bonds –amount of energy released when bonds are broken
• If answer is + - endothermic reaction
(the product is colder than the reactants)
• If answer is - - exothermic reaction
(the product is hotter than the reactants)
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• The following possible values are given for potential energies that are absorbed and released for a reaction.
• Calculate the energy change and determine whether the reaction is exothermic or endothermic.
Examples
Energy absorbed tobreak bonds(𝑘𝐽.𝑚𝑜𝑙−1)
Energy absorbed to
release bonds(𝑘𝐽.𝑚𝑜𝑙−1)
Energy change
(𝑘𝐽.𝑚𝑜𝑙−1)
Endothermic or exothermic
(𝑘𝐽.𝑚𝑜𝑙−1)
350 420
870 630
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Examples•𝐶𝐶𝑙4 𝑔 + 2𝐹2 → 𝐶𝐹4 𝑔 + 2𝐶𝑙2 𝑔 + 752kJ
Exothermic or endothermic ?
Energy is released - hotter
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Examples
•𝐶𝑙𝐹3 g + 514kJ → 𝐶𝑙 𝑔 + 3𝐹(𝑔)
Exothermic or endothermic ?
Energy is absorbed - colder
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Homework
EXERCISE 15 pg. 160-161