Advertisements
Advertisements
प्रश्न
Explain the following reaction with the balanced equation.
Sodium burns in air
Advertisements
उत्तर
On burning, sodium metal combines with oxygen in the air to form sodium oxide.
\[\ce{\underset{\text{Sodium}}{4Na_{(s)}} + \underset{\text{Oxygen}}{O_{2(g)}} -> \underset{\text{Sodium oxide}}{2Na2O_{(s)}}}\]
APPEARS IN
संबंधित प्रश्न
Give one example each of which illustrates the following characteristics of a chemical reaction:
evolution of a gas
How will you obtain Magnesium oxide from magnesium.
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.
Electrolysis of alumina is done.
Divide the metals Cu, Zn, Ca, Mg, Fe, Na, Li into three groups, namely reactive metals, moderately reactive metals and less reactive metals.
State what is meant by the ‘reactivity series of metals’
With reference to Water explain with suitable examples of how the reactivity of the metals could be differentiated.
With reference to Acid explain with a suitable example of how the reactivity of the metals could be differentiated.
Give a balanced equation for the reversible catalytic reaction involving nitrogen as one of the reactants.
Select the correct answer for the statement given below:
The catalyst used in the catalytic reaction involving the reactants nitrogen and hydrogen.
In preparation of Aqua regia hydrochloric acid and _______ acid are mixed.
Classify the following metals based on their reactivity.
Cu, Zn, Ca, Mg, Fe, Na, Li, Hg
| More reactive | Moderately reactive | Less reactive |
Which of the following is the correct arrangement of the given metals in ascending order of their reactivity?
Zinc, Iron, Magnesium, Sodium
A metal that exists as a liquid at room temperature is obtained by heating its sulphide in the presence of air. Identify the metal and its ore and give the reaction involved.
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.
A solution of CuSO4 was kept in an iron pot. After few days the iron pot was found to have a number of holes in it. Explain the reason in terms of reactivity. Write the equation of the reaction involved.
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?
