fill out the table below based on the following chemical equation: __xe+ __f₂→ __xef₆\ntotal # before…
fill out the table below based on the following chemical equation: __xe+ __f₂→ __xef₆\ntotal # before (reactants) | elements | total # after (reactants)\n| | xe | |\n| | f | |\nthe correct coefficients for the equation is: __xe + __f₂→ __xef₆
Answer
Explanation:
Step1: Balance the equation
We need to make the number of each element on the reactant side equal to that on the product side. For the reaction $\text{Xe}+\text{F}_2\rightarrow\text{XeF}_6$, we have 1 Xe on the left - hand side and 1 Xe on the right - hand side. For fluorine, we have 2 F atoms in $\text{F}_2$ and 6 F atoms in $\text{XeF}_6$. To balance the F atoms, we need 3 moles of $\text{F}_2$. So the balanced equation is $\text{Xe} + 3\text{F}_2\rightarrow\text{XeF}_6$.
Step2: Count the number of atoms before and after
Before the reaction (reactants): For Xe, the total number is 1; for F, since we have 3 moles of $\text{F}_2$, the total number of F atoms is $3\times2 = 6$. After the reaction (products): For Xe, in 1 mole of $\text{XeF}_6$, the number of Xe atoms is 1; for F, in 1 mole of $\text{XeF}_6$, the number of F atoms is 6.
Answer:
| Total # Before (reactants) | Elements | Total # After (Reactants) |
|---|---|---|
| 1 | Xe | 1 |
| 6 | F | 6 |
| The correct coefficients for the equation is: 1 Xe + 3 $\text{F}_2$ → 1 $\text{XeF}_6$ |