# Chapter 4 - Reactions in Aqueous Solution - Exercises - Page 159: 4.53a

$Mn_{(s)}+H_{2} SO_{4(aq)}-->MnSO_{4(aq)}+H_{2(g)}$ molecular, $Mn_{(s)}+2H_{(aq)}^{+}-->Mn_{(aq)}^{2+} +H_{2(g)}$ net ionic.

#### Work Step by Step

Start by writing down the different elements and ions from the reactants individually: $Mn_{(s)}, H_{(aq)}^{+}, SO_{4(aq)}^{2-}, H_{2}O_{(l)}$. Upon reaction with acids, metals form salts and hydrogen gas. The question also indicates that the sulfuric acid is dilute, therefore the reaction will produce no water. $Mn_{(s)}+H_{2} SO_{4(aq)}-->MnSO_{4(aq)}+H_{2(g)}$ Since the molecular equation is already balanced, there are no further steps required for solving this part. For the net ionic equation, we will focus only on what happens to the ions in the reaction. Cancel out all ions that don’t change between reactants and products: $Mn_{(s)}+2H_{(aq)}^{+}+ SO_{4(aq)}^{2-}-->Mn_{aq}^{2+} + SO_{4(aq)}^{2-}+H_{2(g)}$ $SO_{4(aq)}^{2-}$ is a spectator ion, as it is common between both sides of the reaction. We are left with: $Mn_{(s)}+2H_{(aq)}^{+}-->Mn_{(aq)}^{2+} +H_{2(g)}$ as the net ionic reaction.

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