Balance the following chemical equations: a. _ KO (s) + _ H
O (l) ? _ KOH (aq) + _ O
(g) + __ H
O
(aq)
The Correct Answer and Explanation is:
To balance the chemical equation:
__KO (s) + __H₂O (l) → __KOH (aq) + __O₂ (g) + __H₂O (aq)
Start by identifying the atoms on both sides of the equation.
Unbalanced:
- Reactants: KO, H₂O
- Products: KOH, O₂, H₂O
To balance:
- Potassium (K) appears once on both sides, so it remains unchanged.
- Oxygen (O) appears in multiple compounds, requiring careful balancing.
- Hydrogen (H) is present in water molecules, which need adjustment.
Balanced equation: 2 KO (s) + H₂O (l) → 2 KOH (aq) + O₂ (g)
Explanation:
Balancing chemical equations ensures that the number of atoms for each element remains the same on both sides. The reaction starts with potassium monoxide (KO) reacting with water (H₂O) to produce potassium hydroxide (KOH) and oxygen gas (O₂).
Initially, the unbalanced equation shows unequal oxygen atoms. Oxygen in KO and H₂O must match the number in the products. Since molecular oxygen (O₂) forms in diatomic pairs, coefficients need adjustment to achieve balance.
Potassium is already balanced at the start, appearing once on both sides. Water molecules contribute hydrogen and oxygen atoms, affecting the final coefficients. Adding the appropriate number of KO units ensures an equal distribution. The balanced equation results from adjusting the coefficients so that each element has the same quantity on both sides.
This approach follows the principle of conservation of mass, confirming that no atoms are lost or created. By applying logical adjustments, the final equation reflects a properly balanced reaction.
