During preparation of `XeF_4` from Xenon and Fluorine, these two elements are reacted in which of the following given ratios ?

Options

A. Xenon (1) Fluorine (Excess)
B. Xenon (1) Fluorine (5)
C. Xenon (1) Fluorine (20)
D. Xenon (1) Fluorine (4)

Answer

To determine the ratio in which xenon (Xe) and fluorine (F2) react to form xenon tetrafluoride (XeF4), we need to analyze the chemical reaction involved in the formation of this compound.

### Step-by-Step Solution:

1. **Write the Chemical Equation**:
The reaction for the formation of xenon tetrafluoride can be represented as:
\[ \text{Xe} + 2 \text{F}_2 \rightarrow \text{XeF}_4 \]

2. **Identify the Reactants and Products**:
- Reactants: Xenon (Xe) and Fluorine (F2)
- Product: Xenon tetrafluoride (XeF4)

3. **Determine the Stoichiometric Coefficients**:
From the balanced chemical equation, we see that:
- 1 mole of xenon (Xe) reacts with 2 moles of fluorine (F2) to produce 1 mole of xenon tetrafluoride (XeF4).

4. **Establish the Reaction Ratio**:
The ratio of xenon to fluorine in the reaction is:
\[ \text{Ratio of Xe to F2} = 1:2 \]

### Final Answer:
The elements xenon and fluorine react in the ratio of **1:2** during the preparation of XeF4.

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