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→Finding the Empirical Formula
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State the [[mass]] of all [[reactant]]s.
[[Mass]] of [[Oxygen]] = 64g
[[Relative Atomic Mass]] of [[Oxygen]] = 16g
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State the [[mass]] of all [[reactant]]s.
[[Mass]] of [[Carbon]] = 60g
[[Relative Atomic Mass]] of [[Carbon]] = 12g
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State the [[mass]] of all [[reactant]]s.
[[Mass]] of [[Sulphur]] = 416g
[[Relative Atomic Mass]] of [[Sulphur]] = 32g
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Find the number of [[mole]]s of each [[element]].
[[Mole]]s of [[Oxygen]] = 64/16
[[Mass]] of [[Hydrogen]] = 8g
[[Relative Atomic Mass]] of [[Hydrogen]] = 1g
[[Mole]]s of [[Hydrogen]] = 8 mole
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[[Mole]]s of [[Carbon]] = 60/12
[[Mass]] of [[Oxygen]] = 160g
[[Relative Atomic Mass]] of [[Oxygen]] = 16g
[[Mole]]s of [[Oxygen]] = 10 mole
| style="height:20px; width:200px; text-align:left;" |Find the number of [[mole]]s of each [[element]]. [[Mole]]s of [[CarbonSulphur]]:= 416/32 [[Mole]]s of [[OxygenSulphur]]= 32 mole
[[MassMole]] s of [[SulphurOxygen]] = 416g26 mole
|-| style="height:20px; width:200px; text-align:left;" |Find the [[Relative Atomic Mass]] of [[SulphurRatio]] = 32g:
[[MoleHydrogen]]s of :[[SulphurOxygen]] = 416/32
2:1| style="height:20px; width:200px; text-align:left;" |Find the [[Mass]] of [[OxygenRatio]] = 416g:
[[Relative Atomic MassCarbon]] of :[[Oxygen]] = 16g
1:2| style="height:20px; width:200px; text-align:left;" |Find the [[Mole]]s of [[OxygenRatio]] = 26 mole:
[[Sulphur]]:[[Oxygen]]
1:2
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| style="height:20px; width:200px; text-align:left;" |The '''empirical formula''' of the [[product]] is H<sub>2</sub>O
| style="height:20px; width:200px; text-align:left;" |The '''empirical formula''' of the [[product]] is SOCO<sub>2</sub>
| style="height:20px; width:200px; text-align:left;" |The '''empirical formula''' of the [[product]] is SO<sub>2</sub>
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