How to Ensure Safety During Chemical Experiments with Metals

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Explore the calculation of synthetic ruby’s empirical formula, Gay-Lussac’s gas laws, safety in metal reactivity, and why aluminium remains vital in industry.

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Our team of top specialists in chemistry and industrial applications has developed this slide file to simplify complex ideas. Each slide focuses on key learning points, making concepts such as chemical reactions, empirical formulas, and industrial uses of metals easy to understand. We use plain language and engaging visuals to explain detailed processes step by step. This approach makes learning both effective and enjoyable.

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Additional information

Metals

Question 35
Artificial rubies can be manufactured and on analysis are
found to contain 52.9% aluminium and 47.1% by mass of
oxygen. The traces of an oxide of chromium were ignored in
the analysis. Find the empirical formula of the compound.
In 100 g, the ratio
1 1
52.9 g 47.1 g AI: O :
26.98 g mol 16 g mol  
   
        
In 100 g, the ratio
AI:O1.96: 4 2.9
Divide by the smallest number
 1.96 / 1.96 : 2.94 / 1.96   
Divide by the smallest number
1:1.5 so ratio 2: 3 Thus the empirical formula is Al2O3

Question 36
Describe the contribution of Gay-Lussac to the
understanding of gaseous reactions.
When the volumes of gases involved in a chemical reaction
are measured at the same temperature and pressure, the
volume ratios are simple whole numbers.

Question 37
In this topic, you carried out a first-hand investigation to
compare the relative reactivity of metals. Describe the safety
precautions you took.
The safety precautions that were taken included:
 Using tongs to handle metal samples
 Wearing goggles to prevent splashing acid into eyes
 Wearing gloves to prevent acid splashing on to hands
 Working in a well-ventilated area

Question 38
A mixture of 10 g of iron filings and 10 g of sulfur is heated to
its reaction temperature. How many grams of FeS is formed.
Since the ratio of reactants is one to one, the Fe is the
limiting reagent.
Therefore 0.179 mol of FeS is formed.
m n MM 0.179 55.85 32.06 FeS FeS FeS       
FeS m 15 g

Question 39
Explain why the production of aluminium is continued
despite the huge energy requirements and high price
compared to iron.
Aluminium is an extremely useful metal to industry.
Its low density and high strength make it ideal for many high
speed applications like jet aircraft.
Additionally the high electrical conductivity makes
aluminium useful in electrical wiring systems where weight is
a consideration.
With all these industrial applications the high cost of
aluminium is offset by the number of applications it has.
This is why the production of aluminium has continued so
steadily despite its high cost and energy input.