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Cannot use this method

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heating, weighing and cooling process is repeated with until a constant mass is obtained.

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Hi cherr

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To eliminate all the air in the apparatus 

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To eliminate all the air in the apparatus 

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Molecular formula is a formula that shows the actual number of atoms of each element that are present in a compound.

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Lead (II) is less reactive towards oxygen.
(not sure cher)

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a) Empirical formula is a chemical formula that shows the simplest whole number ratio of atoms of each element in a compound

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Idk this one teacher

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Empirical formula is a chemical formula that shows the simplest whole number ratio of number of atoms in each element in a compound

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2 information that can be interpreted from the chemical equation:
4 moles of Aluminium reacts with 3 moles of oxygen to produce 2 moles of aluminium oxide

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To allow to oxygen to enter and react with metal X.

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Interpret the chemical equation qualitatively and quantitatively.

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Interpret the chemical equation qualitatively and quantitatively.

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Qualitative - The reactants are solid iron and oxygen gas. The product is solid Iron (iii) oxide.
Quantitative - 4 moles of Fe reacts with 3 moles of O2 to produce 2 moles of Fe2O3

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Empirical formula is a chemical formula that shows the simplest whole number ratio of atoms of each element present in a compound

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Empirical formula is a chemical formula that shows the simplest whole number ratio of number of atoms in each element in a compound

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an ion is formed

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Hydrogen gas

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State how to determine that the reaction between X and oxygen has completed

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State how to determine that the reaction between X and oxygen has completed

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Heating, cooling and weighing process until constant mass is obtained

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empirical formula is a chemical compound which is the simplest ratio of atoms in a compound.

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I am not sure Cher :(

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HAGHSGDHAGSDASHKSAUHF O ME GODD

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4Fe(s) + 3O2 (g) -> 2Fe2O3 (s)

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When carrying out in this experiment, why does the crucible lid need to be opened once in a while?

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When carrying out in this experiment, why does the crucible lid need to be opened once in a while?

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To let the oxygen to enter the crucible to react with magnesium ribbon.

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im not sure cher : ]

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Reactants : K, H20
Products : KOH, H2

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to test if hydrogen gas is present

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CuO + H2 ---> Cu + H2O

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It is because zinc is more reactive towards hydrogen

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magnesium: 27.75 - 25.35 = 2.4g
oxygen: 29.35 - 27.75 = 1.6g

n.o.m of magnesium atom = 2.4/24 = 0.1 mol
n.o.m of oxygen atom = 1.6/16 = 0.1 mol

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x : 2
y: 2
z : 2

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Copper (II) Oxide

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Amount of substance that contains as many particles as the number of atoms in exactly 12 gram of carbon-12

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2moles of K reacts with 2 moles of H2O to produce 2moles of KOH and 1 mole of H2

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Magnesium
n=m/M
n=2.4g/24
n=0.1
=0.1/0.1
SROM=1

Oxygen
n=m/M
n=1.6g/16
n=0.1
=0.1/0.1
SROM=1

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Acts as an reducing agent

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empirical formula is a chemical formula that shows the simplest whole number ratio of atom of each emlement in a compound

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Magnesium is a reactive metal

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heating, cooling and weighing process are repeated until a constant mass is obtained

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magnesium is more reactive than hydrogen

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The empirical formula of magnesium oxide is MgO

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The empirical formula of magnesium oxide is MgO

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No because copper does not easily react with oxygen.

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Flow hydrogen gas to remove all air

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Nice tryyy! kipidap dongibap

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dashyat

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Flow dry hydrogen in a few minutes to eliminate all the oxygen gas in combustion tube

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RASHmika will be proud

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copper = 7.2/64
= 0.1125
oxygen = 0.8/16
= 0.05

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u got this bossku. Kipidap dongibap!

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b) Hydrogen gas is used in this experiment. Name one of the chemical used to prepare the hydrogen gas.

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b) Hydrogen gas is used in this experiment. Name one of the chemical used to prepare the hydrogen gas.

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Zinc / Sulphuric acid
(not sure teacher😬)

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Cu2O

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Mg,Magnesium.Because it is more reactive than hydrogen

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empirical formula is a chemical formula that that shows the simplest ratio of number of atoms of each element in a compound

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mass of copper : 7.2 g
mass of oxygen : 0.8 g

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to ensure all the oxygen has been removed

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powerrr !

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EF : LO

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EF : LO