Advertisements
Advertisements
प्रश्न
Write chemical equation for the event.
Iron filings are dropped in aqueous solution of copper sulphate.
Iron dissolved in aqueous solution of copper sulphate.
Advertisements
उत्तर
Iron displaces copper from copper sulphate solution forming ferrous sulphate and copper.
\[\ce{\underset{\text{Iron}}{Fe_{(s)}} + \underset{\text{Copper sulphate}}{CuSO_{4(aq)}} -> \underset{\text{Ferrous sulphate}}{FeSO_{4(aq)}} + \underset{\text{Copper}}{Cu_{(s)}}}\]
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?
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 a chemical equation for the following event.
Zinc oxide is dissolved in dilute hydrochloric acid.
With reference to Water explain with suitable examples 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.
Complete the statement by filling in the blank with the correct word:
The metal which reacts with steam and the reaction is reversible is ________.
Explain the following reaction with the balanced equation.
Reaction of aluminium with oxygen
Explain the following reaction with the balanced equation.
Magnesium reacts with dil HCl
Which among the following alloys contain mercury as one of its constituents?
A metal A, which is used in thermite process, when heated with oxygen gives an oxide B, which is amphoteric in nature. Identify A and B. Write down the reactions of oxide B with HCl and NaOH.
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.
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.
Give the steps involved in the extraction of metals of low and medium reactivity from their respective sulphide ores.
Of the three metals X, Y and Z. X reacts with cold water, Y with hot water and Z with steam only. Identify X, Y and Z and also arrange them in order of increasing reactivity.
Metal ‘A’ has electronic configuration 2, 8, 1 and metal ‘B’ has electronic configuration 2, 8, 8, 2. Out of these, which metal is more reactive? Write the reaction of this metal with dilute HCl acid.
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?
