Complete and balance each equation. If no reaction occurs, write 'NO REACTION.' c. CrBr₂(aq) + Na₂CO₃(aq) →

Verified step by step guidance

1. Identify the reactants: CrBr_2 (aq) and Na_2CO_3 (aq).
2. Determine the possible products by considering the exchange of ions: CrCO_3 and NaBr.
3. Check the solubility of the products: CrCO_3 is insoluble in water, while NaBr is soluble.
4. Write the balanced chemical equation: CrBr_2 (aq) + Na_2CO_3 (aq) → CrCO_3 (s) + 2 NaBr (aq).
5. Verify the balance of atoms and charges on both sides of the equation.

Key Concepts

Balancing Chemical Equations

Balancing chemical equations involves ensuring that the number of atoms of each element is the same on both sides of the equation. This is based on the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. To balance an equation, coefficients are adjusted in front of the chemical formulas to achieve equal atom counts.

Types of Chemical Reactions

Understanding the types of chemical reactions is crucial for predicting the products of a reaction. Common types include synthesis, decomposition, single replacement, and double replacement reactions. In the given equation, recognizing that CrBr₂ and Na₂CO₃ may undergo a double replacement reaction helps in determining the potential products and whether a reaction will occur.

Solubility Rules

Solubility rules help predict whether a compound will dissolve in water or form a precipitate. For example, most bromides are soluble, but some metal bromides may not be. In this case, knowing the solubility of the reactants and potential products is essential to determine if a reaction occurs or if 'NO REACTION' is the appropriate conclusion.