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 that reacts, what mass of water is requiered?
b)If the three reactions occur in sequence, for each 0.250 grams of xenon that reacts, what is the theoretical yield of hydrogen flouride in grams?
c)If 0.123 moles of xenon flouride reacts with 0.333moles of water, what mass of hydrogen flouride forms?
a)
Convert 0.0250 g XeF6 to moles. moles = grams/molar mass.
Convert moles XeF6 to moles H2O.
moles XeF6 x (1 mole H2O/1 mole XeF6) = mol XeF6 x 1 = ?
Then convert moles H2O to grams. g = moles x molar mass.
b)You CAN work three stoichiometry problems here; i.e., 0.250 g Xe and convert to g XeF2, then use that to convert to g XeF6, then again to convert XeF6 to HF. But you can cut out all of the middle work this way.
Go through the reactions mole for mole like this.
1 mole Xe = 1 mol XeF2 = 1 mol XeF6 = 6 mol HF; therefore, we know 1 mol Xe = 6 mol HF.
mol Xe = 0.250/atomic mass Xe
Convert mol Xe to mol HF like this.
moles Xe x (6 mol HF/1 mol Xe) = mole Xe x (6/1) = ?
Then convert moles HF to grams. g = mols x molar mass. That is the theoretical yield of HF in grams. You an see this is just another stoichiometry problem.
c. This is a limiting reagent problem. I'll leave that for you. Post your work if you get stuck.
To answer these questions, we'll use stoichiometry, which is a way of determining the quantities of substances involved in chemical reactions.
a) For each 0.0250 grams of xenon hexafluoride (XeF6) that reacts, we need to find the mass of water (H2O) required. Here's how you can calculate it:
1. Determine the molar mass of XeF6:
Xenon (Xe) has an atomic mass of 131.29 g/mol, and fluorine (F) has an atomic mass of 18.998 g/mol. Since there are six fluorine atoms in XeF6, the molar mass of XeF6 is:
Molar mass of XeF6 = (1 * molar mass of Xe) + (6 * molar mass of F)
2. Calculate the number of moles of XeF6:
Number of moles of XeF6 = Mass of XeF6 / Molar mass of XeF6
3. Use the stoichiometry of the reaction to determine the ratio of moles of XeF6 to moles of H2O:
From the balanced chemical equation:
1 mole of XeF6 reacts with 1 mole of H2O
4. Calculate the mass of water required:
Mass of H2O = Number of moles of XeF6 * Molar mass of H2O
b) If the three reactions occur in sequence, and for each 0.250 grams of xenon (Xe) that reacts, we need to find the theoretical yield of hydrogen fluoride (HF) in grams. Here's how to calculate it:
1. Determine the molar mass of Xe:
Molar mass of Xe = Atomic mass of Xe
2. Calculate the number of moles of Xe:
Number of moles of Xe = Mass of Xe / Molar mass of Xe
3. Use the stoichiometry of the reactions to find the ratio between moles of Xe and moles of HF in each reaction.
From the first reaction:
1 mole of Xe reacts with 2 moles of F2 to produce 1 mole of XeF2
From the second reaction:
1 mole of XeF2 reacts with 2 moles of F2 to produce 1 mole of XeF6
From the third reaction:
1 mole of XeF6 reacts with 1 mole of H2O to produce 6 moles of HF
4. Calculate the moles of HF:
Moles of HF = (Number of moles of Xe * 1 * 2 * 1 * 1 * 6)
5. Calculate the mass of HF:
Mass of HF = Moles of HF * Molar mass of HF
c) If 0.123 moles of xenon fluoride (XeF) reacts with 0.333 moles of water (H2O), we need to find the mass of hydrogen fluoride (HF) formed. Here's how to calculate it:
1. Use the stoichiometry of the third reaction:
1 mole of XeF6 reacts with 1 mole of H2O to produce 6 moles of HF
2. Calculate the moles of HF produced using the mole ratios:
Moles of HF = (0.123 moles of XeF6 * 6 moles of HF) / 1 mole of XeF6
3. Calculate the mass of HF:
Mass of HF = Moles of HF * Molar mass of HF
Remember to consult the periodic table for the molar masses of each element involved.
By following these steps, you can determine the mass of water required in reaction a), the theoretical yield of hydrogen fluoride in reaction b), and the mass of hydrogen fluoride formed in reaction c).