Question

The ratio of Xe: \( \text{F}_2 \) required in the above reaction is: \[ \text{Xe}(g) + 2\text{F}_2(g) \xrightarrow{873 \, K, 7 \, \text{bar}} \text{XeF}_4(s) \]

• A. \( 1:2 \)
• B. \( 1:5 \)
• C. \( 1:20 \)
• D. \( 1:12 \)

Hint:

- Xenon reacts with fluorine to form different fluorides, such as XeFsubscript{2}, XeFsubscript{4}, and XeFsubscript{6}.
- The ratio of reactants depends on the conditions such as temperature and pressure.

Answer 1

The Correct Option is B

Step 1: Understanding the Given Reaction - The reaction provided is: \[ Xe(g) + 2F_2(g) \xrightarrow{873 K, 7 { bar}} XeF_4(s) \] - Here, 1 mole of Xenon reacts with 2 moles of Fluorine gas to form XeFsubscript{4}. 
Step 2: Analyzing the Ratio - The ratio of Xe to Fsubscript{2} in the equation is 1:2.
- However, in an extended fluorination process, more fluorine gas may be required to sustain and complete the reaction. 
Step 3: Applying Stoichiometry - From experimental data, the reaction sometimes requires 1:5 (Xe:Fsubscript{2}) under certain conditions.
- This is because excess fluorine helps drive the reaction forward.