Chemistry

posted by .

Xenon of mass 5.08 g reacts with fluorine to form 9.49 g of a xenon fluoride. What is the empirical formula of this
compound?
A) XeF6
B) XeF4
C) XeF2
D) XeF
E) Xe2F

I am not familiar with these types of empirical formula problems. If I'm given the percentages of the elements in the compound, I know what to do, but I have no idea what to do here.

Thanks!

  • Chemistry -

    Oh, and the answer is A. I just don't understand how you get it.

  • Chemistry -

    This is very like the percentage problems. A useful way to do the percentage problems is to follow the steps

    1. Percentages (make sure they add up to 100)
    2. masses (assuming 100 g total so numerically same as percentages)
    3. convert mass to moles (by dividing by relative atomic mass)
    4. divide by smallest number of moles (which gives ratio of the atoms for empirical formula)

    here we have the masses so start at step 3.

  • Chemistry -

    If I don't know the empirical formula, what am I supposed to use for the relative atomic mass here for xenon fluoride to get moles?

  • Chemistry -

    Never mind! :) I think I see what I need to do. I simply subtract the initial mass from the mass of the compound to get the mass of the Chlorine and go from there. Correct?

  • Chemistry -

    Yes, subtract the two so you have

    F Xe
    4.41 g 5.08 g

    Number of moles?

    Divide by smallest.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. chemistry

    In a sealed vessel xenon tetrafluoride, XeF4, reacts with hydrogen gas to give xenon gas and hydrogen fluoride gas. What is a balanced chemical equation, including state symbols, for this reaction. thankyou.
  2. Science (Chemisty)

    Scientists in 1962 became very excited when they were able to create xenon tetrafluoride. Why was this an unusual feat?
  3. Chemistry

    To an initially evacuated 50.0L container maintained at 155C were added 3.20g of gaseous xenon and 4.00g of gaseous fluorine. A spark was used to initiate reaction between xenon and fluorine, and gaseous xenon hexafluoride was the …
  4. Chemistry

    Xe(g) + F2(g) ----uv light---> Xe F2(s) XeF2(g) + 2F2(g) ---catalyst---> XeF6(s) XeF6(s) + H2O(l) ------> Xe O3(s) + 6HF(g) Looking at these three reactions respond the following: a) For each 0.0250 grams of xenon hexaflouride …
  5. CHEMESTRY

    One of the few xenon compounds that form is cesium xenon heptafluoride (CsXeF7). How many moles of CsXeF7 can be produced from the reaction of 13.0 mol cesium fluoride with 14.0 mol xenon hexafluoride?
  6. CHEMESTRY

    One of the few xenon compounds that form is cesium xenon heptafluoride (CsXeF7). How many moles of CsXeF7 can be produced from the reaction of 13.0 mol cesium fluoride with 14.0 mol xenon hexafluoride?
  7. Chemistry

    Calculate the number of grams of xenon in 3.566 g of the compound xenon tetrafluoride.
  8. Chemistry

    Calculate the number of grams of xenon in 3.566 g of the compound xenon tetrafluoride.
  9. Chemistry

    Using the balanced equation below, how many grams of cesium fluoride would be required to make 73.1 g of cesium xenon heptafluoride?
  10. Chem

    When 5.49 g of platinum reacts with an excess of fluorine, 7.65 g of platinum(_) fluoride forms. a. What is the mass of fluorine in the compound?

More Similar Questions