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सी.आई.एस.सी.ई.आईसीएसई ICSE Class 8

How Will You Obtain Magnesium Oxide from Magnesium. Also Give Balanced Equations for the Reactions - Chemistry

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प्रश्न

How will you obtain Magnesium oxide from magnesium.

Also give balanced equations for the reactions

एक पंक्ति में उत्तर

उत्तर

Magnesium when burnt in air (oxygen) Magnesium oxide is formed

\[\ce{2Mg + O2->[heat]  2Mgo}\]

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अध्याय 6: Chemical Reactions - Exercise 2 [पृष्ठ ८६]

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सेलिना Concise Chemistry [English] Class 8 ICSE
अध्याय 6 Chemical Reactions
Exercise 2 | Q 6.1 | पृष्ठ ८६

संबंधित प्रश्न

How will you obtain Zinc chloride from zinc.

Also give balanced equations for the reactions


What is meant by the metal reactivity series ? State its importance, (any two points).


Write chemical equation for the event.

Iron filings are dropped in aqueous solution of copper sulphate.


Write the chemical equation for the event.

A reaction was brought about between ferric oxide and aluminum.


Give a balanced equation for the following type of reaction:

A displacement reaction in which a metal above hydrogen in the reactivity series, displaces another metal from the solution of its compound.


Classify the following metals based on their reactivity.
Cu, Zn, Ca, Mg, Fe, Na, Li, Hg

More reactive Moderately reactive Less reactive
     
     

Explain the following reaction with the balanced equation.

Reaction of aluminium with oxygen


An element A reacts with water to form a compound B which is used in white washing. The compound B on heating forms an oxide C which on treatment with water gives back B. Identify A, B and C and give the reactions involved.


Explain the following

  1. Reactivity of Al decreases if it is dipped in HNO3
  2. Carbon cannot reduce the oxides of Na or Mg
  3. NaCl is not a conductor of electricity in solid state whereas it does conduct electricity in aqueous solution as well as in molten state
  4. Iron articles are galvanised.
  5. Metals like Na, K, Ca and Mg are never found in their free state in nature.

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?


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