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Fe + HCl = FeCl3 + H2 is a Single Displacement (Substitution) reaction where two moles of solid Iron [Fe] and six moles of aqueous Hydrogen Chloride [HCl] react to form two moles of aqueous Ferric Chloride [FeCl 3] and three moles of Dihydrogen [H 2] gas.
2Fe + 6HCl = 2FeCl3 + 3H2 is a redox reaction where Fe is oxidized and H is reduced. Fe is a reducing agent (i.e. it lost electrons) and HCl is a oxidizing agent (i.e. it gained electrons).
1 FeCl 3 + 1 H 2 = 1 Fe + 1 HCl For each element, we check if the number of atoms is balanced on both sides of the equation. Fe is balanced: 1 atom in reagents and 1 atom in products.
2Fe + 2HCl = 2FeCl + H2 is a redox reaction where Fe is oxidized and H is reduced. Fe is a reducing agent (i.e. it lost electrons) and HCl is a oxidizing agent (i.e. it gained electrons).
1 Fe + 1 HCl = 1 H 3 + 1 FeCl 2 For each element, we check if the number of atoms is balanced on both sides of the equation. Fe is balanced: 1 atom in reagents and 1 atom in products. H is not balanced: 1 atom in reagents and 3 atoms in products. In order to balance H on both sides we: Multiply coefficient for HCl by 3 1 Fe + 3 HCl = 1 H 3 + 1 ...
Balanced equation. Step 1. Write down the unbalanced equation ('skeleton equation') of the chemical reaction. All reactants and products must be known. For a better result write the reaction in ionic form. Fe + HCl → HFeCl 4 + H 2. Step 2. Separate the redox reaction into half-reactions.
Balancing the equation can be done only by adjusting the coefficients. Step 2 is a balanced element because there is the same number of atoms of in each side of the equation .
