Read the following statements and choose the correct option. Statement I: All metals in the reactivity series can displace hydrogen from dilute acids to form hydrogen gas. Statement II: Metals below hydrogen in the reactivity series do not produce hydrogen gas with dilute acids.
Statement I is false, but Statement II is true.
The activity (reactivity) series is arranged so that any metal placed above hydrogen is more reactive than hydrogen and can therefore displace it from a dilute acid such as HCl or H2SO4, liberating hydrogen gas.
Metals lying below hydrogen in the series, for example copper, silver, mercury and gold, are less reactive than hydrogen; they cannot push hydrogen out of the acid, so no H2 is evolved when they are placed in dilute acids.
Therefore Statement I, which claims that ALL metals can liberate hydrogen from dilute acids, is incorrect, while Statement II, which restricts hydrogen evolution to metals above hydrogen, is correct.
Hence, Statement I is false, but Statement II is true.
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Important Questions from Chemical Reaction
- Which of the following is NOT an example of combination reaction?
- In a redox displacement reaction, if element X loses electrons and element Y gains electrons, then:
- What is the general name of the reaction between an acid and a base?
- When iron filings are mixed with sulfur powder and the mixture is heated, a black substance called iron sulfide is formed. Which statement best describes the changes involved?
- When an iron nail is dipped in copper sulphate solution, which of the following observations confirms that a displacement reaction has occurred?
