Write balanced molecular and net ionic equations for the reactions of (b) dilute sulfuric acid with iron Hint: These reactions produce a gas.

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Identify the reactants: dilute sulfuric acid (H_2SO_4) and iron (Fe).

Write the balanced molecular equation: \( \text{Fe} + \text{H}_2\text{SO}_4 \rightarrow \text{FeSO}_4 + \text{H}_2 \uparrow \).

Separate the aqueous compounds into ions for the complete ionic equation: \( \text{Fe} + 2\text{H}^+ + \text{SO}_4^{2-} \rightarrow \text{Fe}^{2+} + \text{SO}_4^{2-} + \text{H}_2 \uparrow \).

Cancel out the spectator ions (\( \text{SO}_4^{2-} \)) to write the net ionic equation: \( \text{Fe} + 2\text{H}^+ \rightarrow \text{Fe}^{2+} + \text{H}_2 \uparrow \).

Verify that the net ionic equation is balanced in terms of both mass and charge.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Acid-Base Reactions

Acid-base reactions involve the transfer of protons (H+) between reactants. In this case, sulfuric acid (H2SO4) acts as an acid, donating protons to iron (Fe), which can lead to the formation of iron ions and hydrogen gas. Understanding the role of acids and bases is crucial for predicting the products of the reaction.

Balancing Chemical Equations

Balancing chemical equations ensures that the number of atoms for each element is the same on both sides of the equation, adhering to the law of conservation of mass. This process involves adjusting coefficients in front of compounds to achieve balance, which is essential for accurately representing the stoichiometry of the reaction.

Net Ionic Equations

Net ionic equations focus on the species that actually participate in the reaction, omitting spectator ions that do not change during the reaction. This simplification helps to highlight the essential chemical changes occurring, such as the formation of hydrogen gas from the reaction between sulfuric acid and iron.

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Net Ionic Equations

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