How many moles of UF6 would have to be decomposed to provide enough fluorine to prepare 2.14 mol of CF4?

I'm not sure how to solve this problem?
So far all I did is calculate the moles of F in CF4, which is 8.56 moles

2.14 mol CF4 x (4 mol F/1 mol CF4) x (1 mol UF6/6 mol F) = ? mol UF6.

To solve this problem, you will need to use stoichiometry to relate the amount of UF6 decomposed to the amount of fluorine produced. Here are the steps to solve the problem:

Step 1: Write and balance the chemical equation for the decomposition of UF6.
UF6 → U + 3F2

Step 2: Determine the molar ratio between UF6 and F2 from the balanced equation.
From the balanced equation, we can see that 1 mole of UF6 produces 3 moles of F2.

Step 3: Calculate the moles of F2 required to produce 2.14 mol of CF4.
Since each CF4 molecule contains one fluorine atom, the moles of F2 needed will be equal to the moles of CF4.
Therefore, the moles of F2 required = 2.14 mol

Step 4: Use the molar ratio to find the moles of UF6 required.
According to the molar ratio, 1 mole of UF6 produces 3 moles of F2.
So, moles of UF6 required = (moles of F2 required) / (molar ratio)
= 2.14 mol / 3
= 0.713 mol

Therefore, you would need to decompose 0.713 moles of UF6 to provide enough fluorine to prepare 2.14 moles of CF4.

To solve this problem, we need to set up a balanced chemical equation and use stoichiometry to determine the number of moles of UF6 needed.

First, let's write the balanced equation for the reaction.

UF6 -> 2CF4 + 6F2

From the equation, we can see that 1 mole of UF6 produces 6 moles of F2. However, we need to find the moles of UF6 required to produce 2.14 moles of CF4, which means we need to double the number of moles of F2.

So, the stoichiometric ratio is:

1 mole UF6 = 12 moles F2

Now, we can calculate the moles of UF6 needed using the stoichiometric ratio.

moles of UF6 = (moles of F2/12)

Given that the moles of F2 in CF4 is 8.56 moles, we can substitute this value into the equation:

moles of UF6 = (8.56/12) = 0.7133 moles

Therefore, approximately 0.7133 moles of UF6 would have to be decomposed to provide enough fluorine to prepare 2.14 moles of CF4.