Balance the following chemical equations and determine the type of redox reaction for the second equation: 1. HNO3 -> NO2 + O2 + H2O 2. Cl2 + KOH -> KClO3 + KCl + H2O

Let's balance the chemical equations step by step.

1. HNO₃ → NO₂ + O₂ + H₂O

Step 1: Balance the nitrogen atoms.

The number of nitrogen atoms is already balanced on both sides of the equation.

Step 2: Balance the hydrogen atoms.

We have 1 hydrogen atom on the left and 2 on the right. To balance them, we put a coefficient of 1/2 in front of H₂O:

HNO₃ → NO₂ + O₂ + 1/2 H₂O

Step 3: Balance the oxygen atoms.

On the left, we have 3 oxygen atoms. On the right, we have 2 (from NO₂) + 2 (from O₂) + 1/2 (from H₂O) = 4.5 oxygen atoms. Multiply the equation by 4 to get rid of the fraction:

4 HNO₃ → 4 NO₂ + 4 O₂ + 2 H₂O

Now, let's correct the coefficients by recalculating the oxygen on the right side. There are only 2 atoms of oxygen in O2.

Step 2: Balance the hydrogen atoms.

We have 1 hydrogen atom on the left and 2 on the right. To balance them, we put a coefficient of 1/2 in front of H₂O:

HNO₃ → NO₂ + O₂ + 1/2 H₂O

Step 3: Balance the oxygen atoms.

On the left, we have 3 oxygen atoms. On the right, we have 2 (from NO₂) + 2 (from O₂) + 1/2 (from H₂O) = 4.5 oxygen atoms. To balance them, multiply by 2:

2 HNO₃ → 2 NO₂ + O₂ + H₂O

Now, let's check the atoms: N (2 on both sides), H (2 on both sides), O (6 on both sides). So the equation is balanced.

2. Cl₂ + KOH → KClO₃ + KCl + H₂O

Step 1: Determine the oxidation states of each element.

• Cl₂: Oxidation state of Cl is 0
• KOH: Oxidation state of K is +1, O is -2, H is +1
• KClO₃: Oxidation state of K is +1, O is -2, so Cl is +5
• KCl: Oxidation state of K is +1, so Cl is -1
• H₂O: Oxidation state of H is +1, O is -2

Step 2: Identify the elements that are oxidized and reduced.

Chlorine is both oxidized (from 0 in Cl₂ to +5 in KClO₃) and reduced (from 0 in Cl₂ to -1 in KCl). This is a disproportionation reaction.

Step 3: Balance the equation.

Cl₂ + KOH → KClO₃ + KCl + H₂O

To balance this redox reaction, we can use the half-reaction method or the electron balance method. Since chlorine is both oxidized and reduced, let's balance the equation by considering the changes in oxidation states.

Cl₂ → KClO₃ (oxidation, Cl goes from 0 to +5, change of +5)

Cl₂ → KCl (reduction, Cl goes from 0 to -1, change of -1)

To balance the changes, we need 5 times more reduction than oxidation:

Cl₂ → KClO₃

5 Cl₂ → 5 KCl

So, we have:

3Cl₂ + 6KOH → KClO₃ + 5KCl + 3H₂O

Type of Redox Reaction:

The second reaction is a disproportionation (or auto-redox) reaction because the same element (chlorine) is both oxidized and reduced.

Final Answers:

1. Balanced equation: 2 HNO₃ → 2 NO₂ + O₂ + H₂O

2. Balanced equation: 3Cl₂ + 6KOH → KClO₃ + 5KCl + 3H₂O

Type of redox reaction: Disproportionation