Oxygen difluoride can be prepared by bubbling gaseous fluorine into a 0.5 M solution of NaOH 2F2g) + 2 NaOH (a)---OF2(g) + 2 NaF (aq) + H2O(l) OF2 can be used to prepare compounds such as O2AsF6, containing the oxygen cation, O2+, by the following reaction: 4 OF@ + 2 AsF2----- 2 O2AsF6 + 3 F2 If 14 g of F2 is bubbled through 650 mL of 0.500M of NaOH to prepare OF2 with a 78% yield, how much O2AsF6 can be prepared?
The moles of the reactants are calculated:
n NaOH = M * V = 0.5 M * 0.65 L = 0.325 mol
n F2 = g / MM = 14 g / 38 g / mol = 0.368 mol
According to the reaction, the limit reagent is NaOH, the amount of OF2 produced is calculated:
n OF2 = 0.325 mol NaOH * (1 mol OF2 / 2 mol NaOH) * (78/100) = 0.127 mol
The mass of O2AsF6 that can be produced with this amount of OF2 is calculated:
g O2AsF6 = 0.127 mol OF2 * (2 mol OsAsF6 / 4 mol OF2) * (221 g / 1 mol) = 14.03 g
If you liked the answer, please rate it in a positive way, you would help me a lot, thank you.
Oxygen difluoride can be prepared by bubbling gaseous fluorine into a 0.5 M solution of NaOH...
Gaseous iodine pentafluoride, IF5, can be prepared by the reaction of solid iodine and gaseous fluorine: I2(s)+5F2(g)→2IF5(g) A 5.50 −L flask containing 11.0 g I2 is charged with 11.0 g F2, and the reaction proceeds until one of the reagents is completely consumed. After the reaction is complete, the temperature in the flask is 125 ∘C. A) What is the partial pressure of IF5 in the flask? B) What is the mole fraction of IF5 in the flask? C) Draw...
Gaseous iodine pentafluoride, IF,, can be prepared by the reaction of solid iodine and gaseous fluorine: L(s)+5F, (g)+21IF, (g) A 4.80 -L flask containing 9.60 g I2 is charged with 9.60 g F2, and the reaction proceeds until one of the reagents is completely consumed. After the reaction is complete, the temperature in the flask is 125 °C Part A What is the partial pressure of IF, in the flask? VO Ax P= atm Request Answer Submit Part B What...
Question 7 of 24 > Gaseous hydrogen and oxygen can be prepared in the laboratory from the decomposition of gaseous water. The equation for the reaction is 2H,0(g) — 2H,(8) + O2(g) Calculate how many grams of O2(g) can be produced from 61.9 g H,O(g). mass: go,
5) Gaseous iodine pentafluoride, IFs, can be prepared by the reaction of solid iodine and gaseous fluorine: unbalanced equation A 5.00 L, flask containing 10.0 g of I2 is charged with 10.0 g of F2, and the reaction proceeds until one of the reactants is used up (completely consumed). After the reaction is completed, the temperature in the flask is 125. Calculate the pressure inside the flask 5 points
Fe(II) can be precipitated from a slightly basic aqueous solution by bubbling oxygen through the solution, which converts Fe(II) to insoluble Fe(III): 4Fe(OH)+ (aq) + 4OH- (aq) + O2 (g) + 2H2O (l) -----> 4Fe(OH)3 (s) How many grams of O2 are consumed to precipitate all of the iron in 60.0 mL of 0.0450 M Fe(II)? ____g
Nitric acid can be prepared by bubbling dinitrogen pent- Oxide into water N2O5(g)H20(e)2 H*(aq) 2 NO (aq) (a) How many moles of H are obtained when 1.50 L of N2O5 at 25°C and 1.00 atm pressure is bubbled into water? (b) The solution obtained in (a) after reaction is com- plete has a volume of 437 mL. What is the molarity of the nitric acid obtained?
PART ONE: PART TWO: PART THREE: PART FOUR: Gaseous methane (CH4) will react with gaseous oxygen (O2) to produce gaseous carbon dioxide (CO2 and gaseous water (H20). Suppose 13. g of methane is mixed with 13.8 g of oxygen. Calculate the minimum mass of methane that could be left over by the chemical reaction. Round your answer to 2 significant digits A 1.32-g sample of a compound is burned in a bomb calorimeter, producing a temperature change from 20.85 °C...
Small quantities of oxygen can be prepared in the laboratory by heating potassium chlorate, KCIO,(s). The equation for the reaction is 2 KCIO, 2 KCI+ 30, Calculate how many grams of 0, (g) can be produced from heating 68.1 g KCIO,($). mass Iodine is prepared both in the laboratory and commercially by adding Cl, (g) to an aqueous solution containing 2 Nal(aq) + Cl2(8) — 1(s) + 2 NaCl(aq) How many grams of sodium iodide, Nal, must be used to...
1. Glucose, also known as blood sugar has the formula, C6H12O6. a) Write a balanced equation for the combustion of glucose. b) If 3.8 kcal is released by combustion of each gram of glucose, how many kilocalories are released by the combustion of 1.50 mol of glucose? c) What is the minimum amount of energy a plant must absorb to produced 15.0 g of glucose? 2. In the following, does S increase or decrease: a) A drop of ink spreading...
Problem 6: (Mass, Moles, Limiting Reactant, Yields: 15 points) Chlorine gas can be prepared in the laboratory by the reaction of hydrochloric acid with manganese(IV) oxide. 4 HCl(aq) + MnO2 (s) → _MnCl(aq) + 2 H2O(l) + Cl2(g) a. Balance the above equation (2.5 points) b. A sample of 39.5 g MnO2 is added to a solution containing 45.9 g HCl. Determine the limiting reactant (4 points). Circle your final answer (0.5 point). MnO2 is limiting HCI is limiting c....