Write the redox reaction that occurs when a zinc rod is placed in a $H_2SO_4$ solution.
- A$Zn_{(s)} + H_2SO_{4(aq)} \rightarrow ZnSO_{4(aq)} + H_{2_{(g)}}$
- B$Zn_{(s)} + H_2SO_{4(aq)} \rightarrow ZnS_{(s)} + H_2O_{(l)}$
- C$Zn_{(s)} + H_2SO_{4(aq)} \rightarrow ZnO_{(s)} + SO_{2_{(g)}} + H_2O_{(l)}$
- D$Zn_{(s)} + H_2SO_{4(aq)} \rightarrow Zn_{(s)} + H_2SO_{4(aq)}$
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Similar Questions
Consider the following statements:
In the chemical reaction:
$MnO_2 + 4HCl \to MnCl_2 + 2H_2O + Cl_2$
$(1)$ Manganese ion is oxidised
$(2)$ Manganese ion is reduced
$(3)$ Chloride ion is oxidised
$(4)$ Chloride ion is reduced.
Which of these statements are correct?
In the chemical reaction:
$MnO_2 + 4HCl \to MnCl_2 + 2H_2O + Cl_2$
$(1)$ Manganese ion is oxidised
$(2)$ Manganese ion is reduced
$(3)$ Chloride ion is oxidised
$(4)$ Chloride ion is reduced.
Which of these statements are correct?
Medium
View SolutionWhat is the ratio of the stoichiometric coefficient of $N_2H_4$ to $Cl^-$ in the following balanced redox reaction?
$ClO_3^- + N_2H_4 \to NO_3^- + Cl^-$
$ClO_3^- + N_2H_4 \to NO_3^- + Cl^-$
Difficult
View SolutionThe number of moles of acidified $KMnO_4$ required to convert one mole of sulphite ion into sulphate ion is
Medium
View SolutionIn alkaline condition $KMnO_4$ reacts as follows:
$2KMnO_4 + 2KOH \to 2K_2MnO_4 + H_2O + O$
Therefore,its equivalent weight will be:
$2KMnO_4 + 2KOH \to 2K_2MnO_4 + H_2O + O$
Therefore,its equivalent weight will be:
Medium
View SolutionWhich of the following solutions will turn violet when a drop of lime juice is added to it?
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