`KClO_(3)` decomposes to `KCl` and `O_(2)`. If the volume of `O_(2)` obtained in this reaction is 1.12 lit at STP, weight of KCl formed in the reaction is

Options

A. 7.45g
B. 2.48g
C. 4.96g
D. 1.24g

Explanation

To solve the problem of finding the weight of KCl formed when KClO₃ decomposes to KCl and O₂, follow these steps:

### Step 1: Write the balanced chemical equation
The decomposition of potassium chlorate (KClO₃) can be represented by the following balanced equation:
\[ 2 \text{KClO}_3 \rightarrow 2 \text{KCl} + 3 \text{O}_2 \]

### Step 2: Calculate the number of moles of O₂ produced
Given that the volume of O₂ produced is 1.12 liters at STP (Standard Temperature and Pressure), we can calculate the number of moles of O₂ using the molar volume of a gas at STP, which is 22.4 liters per mole.
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