Element 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. What are the possible formulas for the two compounds?
(Multiple choice)
a. XF (for 1st compound) X2F2 (for 2nd)
b.XF2 XF
c.XF2 X2F
d.X2F XF2
e.X2f3 X3F
The second compound has twice the moles of X compared to as the F, Answer b appears to be only answer that meets the criteria. Check my thinking
To determine the formulas of the two compounds formed by the reaction of Element X and fluorine, you can use the concept of stoichiometry. Stoichiometry is based on the principle that the reactants and products of a chemical reaction are related by a balanced chemical equation.
In the first reaction, where 0.480g of X reacts with 1.000g of F, we need to determine the ratio of moles between X and F. To do this, we need to convert the mass of each element to moles using their respective molar masses.
Step 1: Calculate the number of moles of X.
Molar mass of X = mass of X / molar mass of X
Molar mass of X = 0.480g / molar mass of X
Step 2: Calculate the number of moles of F.
Molar mass of F = mass of F / molar mass of F
Molar mass of F = 1.000g / molar mass of F
Step 3: Determine the mole ratio between X and F by dividing the moles of X by the moles of F.
Mole ratio of X to F = (moles of X) / (moles of F)
Repeat steps 1-3 for the second reaction, where 0.960g of X reacts with 1.000g of F.
Once you have determined the mole ratios for both reactions, you can compare them to deduce the possible formulas for the compounds. In this case, if the mole ratio of X to F is approximately 1:1 in both reactions, then the possible formulas for the compounds are XF (for the first compound) and XF2 (for the second compound).
Therefore, based on your analysis, the correct answer is option b. XF (for the first compound) and XF2 (for the second compound).