Let us consider the following reaction :
`KO_(x) + H_(2)O rarr KOH + H_(Y)O_(Z) + O_(2)`
(unbalanced equation )
`KO_(x)` is a chrome yellow powder . What is the value of X ?

Answer

To determine the value of X in the compound KO_(x), we need to analyze the given reaction and the properties of the compound mentioned.

### Step-by-Step Solution:

1. **Identify the Compound**:
The question states that KO_(x) is a chrome yellow powder. The compound that corresponds to this description is potassium superoxide, which is represented as KO2.

2. **Write the Reaction**:
The unbalanced reaction is given as:
\[ KO_x + H_2O \rightarrow KOH + H_YO_Z + O_2 \]
We suspect that KO_x is KO2 based on the description.

3. **Substituting KO2 into the Reaction**:
If we assume KO_x is KO2, we can rewrite the reaction as:
\[ KO_2 + H_2O \rightarrow KOH + H_2O_2 + O_2 \]
Here, potassium superoxide reacts with water to produce potassium hydroxide (KOH), hydrogen peroxide (H2O2), and oxygen gas (O2).

4. **Balancing the Reaction**:
To ensure that the reaction is balanced, we can check the number of atoms on both sides:
- Left side: 1 K, 2 O (from KO2), 2 H, 1 O (from H2O) = 1 K, 3 O, 2 H
- Right side: 1 K (from KOH), 2 H (from H2O2), 2 O (from H2O2), 1 O (from O2) = 1 K, 3 O, 2 H
The equation is balanced.

5. **Conclusion**:
Since KO2 fits the description of a chrome yellow powder and balances the reaction, we conclude that the value of X is 2.

### Final Answer:
The value of X is 2.