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प्रश्न
Explain the following reaction with the balanced equation.
Reaction of aluminium with oxygen
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उत्तर
Aluminium combines with oxygen to form aluminium oxide.
\[\ce{\underset{\text{Aluminium}}{4Al_{(s)}} + \underset{\text{Oxygen}}{3O_{2(g)}} -> \underset{\text{Aluminium oxide}}{2Al2O_{3(s)}}}\]
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संबंधित प्रश्न
Give one example each of which illustrates the following characteristics of a chemical reaction:
evolution of a gas
What do you observe when dilute sulphuric acid is added to granulated zinc?
What do you observe when a few pieces of iron are dropped in a blue solution of copper sulphate?
Fill in the blank
When a piece of copper is added to silver nitrate solution, it turns ............in colour.
How will you obtain Magnesium oxide from magnesium.
Also give balanced equations for the reactions
How will you obtain Silver chloride from silver nitrate.
Also give balanced equations for the reactions
Write chemical equation for the event.
Aluminium came in contact with air.
Write chemical equation for the event.
Iron filings are dropped in aqueous solution of copper sulphate.
With reference to Water explain with suitable examples of how the reactivity of the metals could be differentiated.
Select the correct answer for the statement given below:
A neutral oxide which does not react with an acid or a base to give salt and water.
Complete the statement by filling in the blank with the correct word:
The metal which reacts with steam and the reaction is reversible is ________.
In preparation of Aqua regia hydrochloric acid and _______ acid are mixed.
Explain the following reaction with the balanced equation.
Sulphur burns in air
Which of the following is the correct arrangement of the given metals in ascending order of their reactivity?
Zinc, Iron, Magnesium, Sodium
An element A burns with golden flame in air. It reacts with another element B, atomic number 17 to give a product C. An aqueous solution of product C on electrolysis gives a compound D and liberates hydrogen. Identify A, B, C and D. Also write down the equations for the reactions involved.
Arrange the following as per the instruction given in the bracket:
Al, K, Mg, Ca (decreasing order of its reactivity)
Three metal samples of magnesium, aluminium and iron were taken and rubbed with sandpaper. These samples were then put separately in test tubes containing dilute hydrochloric acid. Thermometers were also suspended in each test tube so that their bulbs dipped in the acid. The rate of formation of bubbles was observed. The above activity was repeated with dilute nitric acid and the observations were recorded.
Answer the following questions:
(i) When the activity was done with dilute hydrochloric acid, then in which one of the test tubes was the rate of formation of bubbles the fastest and the thermometer showed the highest temperature?
(ii) Which metal did not react with dilute hydrochloric acid? Give reason.
(iii) Why is hydrogen gas not evolved when a metal reacts with dilute nitric acid? Name the ultimate products formed in the reaction.
OR
Name the type of reaction on the basis of which the reactivity of metals is decided. You have two metals X and Y. How would you decide which is more reactive than the other?
