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From the electrochemical series, it can be conculded that:
- a)Zn2+ will liberate H2 from 1 M HCI
- b)Ag metal reacts spontaneously with Zn2+
- c)Zn metal will liberate H2 from 1 M HCI
- d)Ag metal will liberate H2 from 1 M HCI
Correct answer is option 'C'. Can you explain this answer?
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From the electrochemical series, it can be conculded that: a)Zn2+ will...
Zn metal is more reactive, while Ag metal is less reactive than H2, So, Zn metal can reduce H+ ions
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From the electrochemical series, it can be conculded that: a)Zn2+ will...
Electrochemical Series:
The electrochemical series ranks various metals and non-metals in order of their reactivity based on their standard electrode potential. It helps predict the direction of spontaneous redox reactions between different substances.
Zn metal in 1 M HCl:
- According to the electrochemical series, Zn is placed above H2 in the reactivity series.
- This means that Zn metal will liberate H2 gas from 1 M HCl solution.
- The reaction will proceed spontaneously as Zn has a higher tendency to lose electrons compared to H+ ions in the acid.
Explanation:
- When Zn metal is added to 1 M HCl, the following reaction takes place:
Zn(s) + 2HCl(aq) -> ZnCl2(aq) + H2(g)
- Here, Zn displaces H2 from the acid solution and forms ZnCl2, liberating hydrogen gas in the process.
- This reaction occurs because Zn has a higher standard electrode potential than H+ ions in the acid, allowing it to displace hydrogen.
Therefore, based on the electrochemical series and the reactivity of Zn metal, it can be concluded that Zn metal will liberate H2 from 1 M HCl.
The electrochemical series ranks various metals and non-metals in order of their reactivity based on their standard electrode potential. It helps predict the direction of spontaneous redox reactions between different substances.
Zn metal in 1 M HCl:
- According to the electrochemical series, Zn is placed above H2 in the reactivity series.
- This means that Zn metal will liberate H2 gas from 1 M HCl solution.
- The reaction will proceed spontaneously as Zn has a higher tendency to lose electrons compared to H+ ions in the acid.
Explanation:
- When Zn metal is added to 1 M HCl, the following reaction takes place:
Zn(s) + 2HCl(aq) -> ZnCl2(aq) + H2(g)
- Here, Zn displaces H2 from the acid solution and forms ZnCl2, liberating hydrogen gas in the process.
- This reaction occurs because Zn has a higher standard electrode potential than H+ ions in the acid, allowing it to displace hydrogen.
Therefore, based on the electrochemical series and the reactivity of Zn metal, it can be concluded that Zn metal will liberate H2 from 1 M HCl.
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From the electrochemical series, it can be conculded that: a)Zn2+ will liberate H2 from 1 M HCI b)Ag metal reacts spontaneously with Zn2+ c)Zn metal will liberate H2 from 1 M HCI d)Ag metal will liberate H2 from 1 M HCICorrect answer is option 'C'. Can you explain this answer?
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