Medium
Observe the following diagram and answer the questions that follow:
$(i)$ Identify the gases evolved at anode and cathode.
$(ii)$ Why are the amounts of gases collected in the two test tubes not of the same volume?
$(iii)$ What type of reaction is this?
$(iv)$ Why should we use salt water?
$(i)$ Identify the gases evolved at anode and cathode.
$(ii)$ Why are the amounts of gases collected in the two test tubes not of the same volume?
$(iii)$ What type of reaction is this?
$(iv)$ Why should we use salt water?
(N/A) $(i)$ $(a)$ At the anode,oxygen gas is evolved.
$(b)$ At the cathode,hydrogen gas is evolved.
$(ii)$ The amounts of gases collected in the two test tubes are not of the same volume because water $(H_2O)$ consists of hydrogen and oxygen in a molar ratio of $2:1$. Thus,twice as much hydrogen gas is produced compared to oxygen gas.
$(iii)$ This reaction is an electrolytic decomposition reaction.
$(iv)$ Pure water is a poor conductor of electricity. Salt water is used to act as an electrolyte,allowing electricity to pass through the solution to facilitate the decomposition of water.
$(b)$ At the cathode,hydrogen gas is evolved.
$(ii)$ The amounts of gases collected in the two test tubes are not of the same volume because water $(H_2O)$ consists of hydrogen and oxygen in a molar ratio of $2:1$. Thus,twice as much hydrogen gas is produced compared to oxygen gas.
$(iii)$ This reaction is an electrolytic decomposition reaction.
$(iv)$ Pure water is a poor conductor of electricity. Salt water is used to act as an electrolyte,allowing electricity to pass through the solution to facilitate the decomposition of water.
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Balance the following chemical equations:
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$(a)$ $KClO_{3} \longrightarrow KCl + O_{2}$
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View SolutionWhen potassium iodide solution is added to a solution of lead $(II)$ nitrate in a test tube,a precipitate is formed.
$(i)$ Write a balanced chemical equation for this reaction.
$(ii)$ What type of reaction is this?
$(i)$ Write a balanced chemical equation for this reaction.
$(ii)$ What type of reaction is this?
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$2 FeSO_{4} \xrightarrow{\text{Heat}} Fe_{2}O_{3} + \dots + \dots$
$2 FeSO_{4} \xrightarrow{\text{Heat}} Fe_{2}O_{3} + \dots + \dots$
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$3 Fe (s) + 4 H_2 O (g) \rightarrow Fe_3 O_4 (s) + 4 H_2 (g)$
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$(i)$ Iron metal is getting oxidised
$(ii)$ Water is getting reduced
$(iii)$ Water is acting as reducing agent
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View Solution$A, B$ and $C$ are three elements which undergo chemical reactions according to the following equations:
$A_{2}O_{3} + 2B \rightarrow B_{2}O_{3} + 2A$
$3CSO_{4} + 2B \rightarrow B_{2}(SO_{4})_{3} + 3C$
$3CO + 2A \rightarrow A_{2}O_{3} + 3C$
Answer the following questions with reasons:
$(a)$ Which element is the most reactive?
$(b)$ Which element is the least reactive?
$(c)$ What is the type of reactions listed above?
$A_{2}O_{3} + 2B \rightarrow B_{2}O_{3} + 2A$
$3CSO_{4} + 2B \rightarrow B_{2}(SO_{4})_{3} + 3C$
$3CO + 2A \rightarrow A_{2}O_{3} + 3C$
Answer the following questions with reasons:
$(a)$ Which element is the most reactive?
$(b)$ Which element is the least reactive?
$(c)$ What is the type of reactions listed above?
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