Sulfur hexafluoride (SF6; molar mass 146.07 g/mol) is a very stable gas. It is formed by direct synthesis from the elements according to the following reaction: S(s) + 3 F2 (g) → SF6 (g)
If 92 grams of SF6 is produced from the reaction of 115 grams of fluorine (molar mass 38.00 g/mol), what is the percentage yield of the reaction?
a. 62%
b. 78%
c. 80%
d. >100%
1)
S(s) + 3 F2 (g) → SF6 (g)
114 g 146.07 g
114 g F2 -----------> 146.07 g SF6
115 g F2 -----------> ??
mass of SF6 produced = 115 x 146.07 / 114
= 147.35 g
actual yield = 92 g
% yield = (actual / theoretical) x 100
= (92 / 147.35) x 100
= 62 %
percentage yield = 62 %
Sulfur hexafluoride (SF6; molar mass 146.07 g/mol) is a very stable gas. It is formed by...
Sulfur hexafluoride can be synthesized by burning sulfur with fluorine. What is the percent yield of the reaction if 73.3 g of sulfur hexafluoride is recovered from the combustion of 21.1 g of sulfur? S8(s) + 24 F2(g) → 8 SF6 (g)
Sulfur hexafluoride is produced by reacting elemental sulfur with fluorine gas. ___ S8(s) + ___ F2(g) ___ SF6(g)What is the percent yield if 18.3 g SF6 is isolated from the reaction of 10.0 g S8 and 30.0 g F2?
19 CH181-01 20330 )> Homework ) Ch 8 Quantities in Chemical Reactions Sulfur and fluorine react to form sulfur hexafluoride according to the reaction shown here. How many mol of F2 are required to react completely with 2.55 mol of S? s(s) + 3 F2(g) > SF6(g) Select one or more: a. 7.65 mol F b. 15.3 mol F2 C. 2.55 mol F2 d. 0.85 mol F2 Next page
11. Sulfur hexafluoride is produced by reacting elemental sulfur with fluorine gas. Sg(s) + 24 F2(g) - 8 SF6(E) What is the percent vield im 18.3 SF is isolated from the reaction of 10.0 Ss and 300 12 a. 40.2% b. 45.89 c. 47.6% d. 54.656 e. 61.0% 12. The reaction of 5.07 g N with 0.722 g H produces 1.27NH. The percent vield of this reaction is indicate the answer choice that best completes the statement or answers the...
5. Elemental sulfur occurs as octatomic molecules, S8. What mass (g) of fluorine gas is needed to react completely with 17.8 g of sulfur to form sulfur hexafluoride?
6. a. Calculate the density of sulfur hexafluoride gas at 709 torr and 23 C. b. Calculate the molar mass of a vapor that has a density of 7.125 g/L at 11 ∘C and 745 torr . c. Calcium hydride, CaH2, reacts with water to form hydrogen gas: CaH2(s)+2H2O(l)→Ca(OH)2(aq)+2H2(g) This reaction is sometimes used to inflate life rafts, weather balloons, and the like, where a simple, compact means of generating H2 is desired. How many grams of CaH2 are needed...
Antimony can react with chlorine gas to give antimonytrichloride. _____ Sb(s) + _____ Cl2(g)?_____ SbCl3(l) Which of the following is the best set of stoichiometric coefficients to balance this equation? (a) 1, 1, 1 (b) 1, 3, 2 (c) 4, 6, 4 (d) 2, 3, 2 (iv) The very stable compound SF6 is made by burning sulfur in an atmosphere of fluorine. S8(s) + 24 F2(g)?8 SF6(g) If you need 2.50 moles of SF6, you will need to use (a)...
The molar mass of AB is 75.0 g/mol, the molar mass of AC is 60.0 g/mol, and the molar mass of B is 50.0 g/mol. What is the theoretical yield (in grams) of AC from the reaction of 28.0 g of AB?
mass is 162 g/mol. What are the empirical anu mom lar formulas of nicotine? etermining Formulas from Mass Data e Examples 2.10 and 2.11.) 3. A compound containing xenon and fluorine was pre- pared by shining sunlight on a mixture of Xe (0.526 g) and excess F2 gas. If you isolate 0.678 g of the new compound, what is its empirical formula? Elemental sulfur (1.256 g) is combined with fluorine, F2, to give a compound with the formula SF,, a...
2Mg(s) + O2(9) --> 2Mgº(s) molar mass Mg = 24.30 g/mol molar masso2 = 31.98 g/mol molar mass Mgo = 40.29 g/mol If 12.6 grams of magnesium completely react to form magnesium oxide according to the equation given, how much magnesium oxide is produced?