for the reaction shown, identify the element oxidized, the element reduced, the oxidizing agent, and the…

for the reaction shown, identify the element oxidized, the element reduced, the oxidizing agent, and the reducing agent.\nkno₃ → kno₂ + o₂\nwhich element is oxidized?\nwhich element is reduced?\nwhat is the oxidizing agent?\nwhat is the reducing agent?

for the reaction shown, identify the element oxidized, the element reduced, the oxidizing agent, and the reducing agent.\nkno₃ → kno₂ + o₂\nwhich element is oxidized?\nwhich element is reduced?\nwhat is the oxidizing agent?\nwhat is the reducing agent?

Answer

Explanation:

Step1: Determine oxidation - states

In $KNO_3$, potassium ($K$) has an oxidation - state of + 1, oxygen ($O$) has an oxidation - state of - 2. Let the oxidation - state of nitrogen ($N$) be $x$. Using the rule that the sum of oxidation states in a neutral compound is 0, we have $(+1)+x + 3\times(-2)=0$, so $x = +5$. In $KNO_2$, potassium ($K$) is + 1, oxygen ($O$) is - 2, and for nitrogen ($N$), $(+1)+x+2\times(-2)=0$, so $x = +3$. In $O_2$, the oxidation - state of oxygen is 0.

Step2: Identify oxidized and reduced elements

Oxygen in $KNO_3$ has an oxidation - state of - 2 and in $O_2$ it is 0. So, oxygen is oxidized (its oxidation state increases). Nitrogen in $KNO_3$ has an oxidation - state of + 5 and in $KNO_2$ it is + 3. So, nitrogen is reduced (its oxidation state decreases).

Step3: Determine oxidizing and reducing agents

The substance that contains the element that is reduced is the oxidizing agent. So, $KNO_3$ is the oxidizing agent as it contains nitrogen which is reduced. The substance that contains the element that is oxidized is the reducing agent. So, $KNO_3$ is the reducing agent as it contains oxygen which is oxidized.

Answer:

Which element is oxidized? Oxygen Which element is reduced? Nitrogen What is the oxidizing agent? $KNO_3$ What is the reducing agent? $KNO_3$