# Elements X and fluorine react to form two different compounds. In the first reaction 0.480g of X reacts with 1.000g of F. In the second, 0.960g of X reacts with 1.000g of F. Which are possible formulas for the two compunds

First Compound Second Compound
a)XF X2F2
b)XF2 XF
c)XF2 X2F
d)X2F XF2
e)X2F3 X3F

## To determine the formulas of the two compounds, we need to find their empirical formulas.

Step 1: Find the moles of each element in both reactions.
In the first reaction:
- Moles of X = 0.480g X / molar mass of X
- Moles of F = 1.000g F / molar mass of F

In the second reaction:
- Moles of X = 0.960g X / molar mass of X
- Moles of F = 1.000g F / molar mass of F

Step 2: Determine the mole ratio between X and F in both reactions.
To find the empirical formula, we need to simplify the mole ratio between X and F to the simplest whole-number ratio.

In the first reaction, the mole ratio between X and F is:
- Moles of X : Moles of F

In the second reaction, the mole ratio between X and F is:
- Moles of X : Moles of F

Step 3: Simplify the mole ratio to the simplest whole-number ratio.
To simplify the mole ratio to the simplest whole-number ratio, you can divide both the moles of X and F by their lowest common value.

Step 4: Determine the empirical formula.
The empirical formula shows the simplest whole-number ratio of the atoms present in the compound.

Based on the simplified mole ratio, we can determine the formulas for the two compounds.

For the first compound, if the mole ratio between X and F is 1:2, the empirical formula would be XF2.

For the second compound, if the mole ratio between X and F is 1:1, the empirical formula would be XF.

Hence, the possible formulas for the two compounds are:
- First Compound: XF2
- Second Compound: XF

Therefore, the correct answer would be (b) XF2 and (f) XF.