Write the balanced equations for the following reactions :
* (iii) `Ag_((s))+HCl_((1))rarrAgCldarrH_(2)uarr`

Explanation

Step 1 : Rewrite the given equation as it is
`Ag_((s))+HCl_((1))rarrAgCldarrH_(2)uarr`
Step 2 : Write the number of atoms of each element in the unbalanced equation on both sides of equations.

The number of silver and chlorine atoms on both sides of the equation are same , therefore ,equalise the number of hydrogen atoms.
Step 3 : To balance the number of hydrogen atoms.

To equalise the number of hydrogen atoms, we use 2 as the factor in the product HCl , now the unbalanced equation become
`Ag+2HClrarrAgCl+H_(2)`
Step 4 : To balnce the number of chlorine atoms :
To equalise the number of chlorine atoms, we use 2 as the factor in the product AgCl, now the unbalnced equation becomes
`Ag+2HClrarr2AgCl+H_(2)`
Now count the atoms of each element on both sides of the reactant. Now equalise the silver atoms , the balanced equation becomes `2Ag+2HClrarr2AgCl+H_(2)`
Now indicate the physical states of the reactants abd products
`2Ag_((s))+2HCl_((1))rarr2AgCldarr+H_(2)uarr`