In the activity series of metals which metals will displace hydrogen from an acid

The metal that will displace hydrogen from an acid is to the left of Hydrogen in the Voltaic series

There are two types of chemical reactions that may occur.

namely single-replacement reactions and double-replacement reactions.

A single replacement reaction is a chemical reaction in which one element replaces the other elements of a compound to produce new elements and compounds

Not all of these reactions can occur. We can use the activity series, which is a list of elements that can replace other elements below / to the right of them in a single replacement reaction.

This series is better known as the Voltaic series, where the metal element with a more negative electrode potential is on the left, while the element with a more positive electrode potential on the right.

The more left the position of a metal in the series, the more reactive metal (easy to release electrons, the stronger the reductor)

Generally, the Voltaic series used is

Li K Ba Sr Ca Na Mg Al Mn Zn Cr Fe Cd Co Ni Sn Pb H Sb Bi Cu Hg Ag Pt Au

Example:

2Al (s) + 3Zn (NO₃) ₂ (aq) → 2Al (NO₃) ₃ (aq) + 3Zn (s)

The existing aluminum element can replace the zinc element, which is Al on the left side of Zn so the reaction will occur

From periodic system :

Metal element:

a. Group IA, except hydrogen

b. Group IIA

c. Group IIIA, except boron

d. Group IIIB-IIB

e. Group IVA = lead and lead

f. Group VA  = bismuth

Nonmetallic elements:

a. Group IA  = hydrogen

b. Group IVA = carbon

c. Group VA  = nitrogen, phosphorus

d. Group VIA = oxygen, sulfur, selenium

e. Group VIIA = Phosphorus, chlorine, Bromine, Iodine

f. Group VIIIA

The metal that will displace hydrogen from an acid is to the left of Hydrogen in the Voltaic series, including:

IA: Li, Na, K

IIA: Ba Sr Ca Mg

IIIA: Al

IIB: Zn, Cd

IVA: Sn Pb

an oxidation-reduction reaction

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a reducing agent during a redox reaction

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loses electrons in a chemical reaction

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3 1/4 %

explanation: