Sulfur dioxide combines with O2 in the presence of a catalyst as represented by the equation 2SO2(8) + O2(8) 2SO3(g) Suppose 0.10 mol of SO, and 0.10 mol of O, are added to a 1-L vessel. At equilibrium, which of the following conditions must be true? O 102) = 2[SO3] O [SO2) = [02] O ISO2) > [02] [SO2) < [O2] O [SO2) = [02] = [SO3]

Sulfur dioxide combines with O2 in the presence of a catalyst as represented by the equation 2SO2(8) + O2(8) 2SO3(g) Suppose 0.10 mol of SO, and 0.10 mol of O, are added to a 1-L vessel. At equilibrium, which of the following conditions must be true? O 102) = 2[SO3] O [SO2) = [02] O ISO2) > [02] [SO2) < [O2] O [SO2) = [02] = [SO3]

EBK A SMALL SCALE APPROACH TO ORGANIC L

4th Edition

ISBN:9781305446021

Author:Lampman

Publisher:Lampman

Chapter13: Isolation Of Eugenol From Clov

Section: Chapter Questions

Problem 9Q

See similar textbooks

Similar questions

A 244.5-g sample of ground water is analyzed for calcium. The Ca2+ in the sample is first precipitated and filtered-off as NH4CaPO4.7H20. This precipitate is dried and heated, releasing water and ammonia to yield anhydrous calcium pyrophosphate (CaP2O7). The mass of CaP2O, obtained is 0.0419 g. Give the calcium content of the ground water in parts per million (to three significant figures).
To prepare a very dilute solution of K2Cr2O7 (294.18 g/mol), 0.661 g of K2Cr2O7 was transferred to a 250.0-mL volumetric flask and adding water to the mark. A sample of this solution of volume 1.000 mL was then transferred to a 500.0-mL volumetric flask and diluted to the mark with water. Subsequently, 10.0 mL of the diluted solution was transferred to a 250.0-mL flask and diluted to the mark with water. What is the final concentration of K2Cr2O7 in this last solution?
When treating a mixture of metals( copper and zinc) with an excess of solution of hydrochloric acid, 2.24 liters of a gas(STP) were released. When the same mixture was treated with phosphoric acid precipitate of 93.5g is formed. Find the mass fraction of metals in the initial mixture.
A salt solution (30% Na2CO3) weighing 1ton iscooled to 20C where the salt crystallizes asdecahydrate. What will be the crystal yield ifthe solubility is 21.5 kg anhydrous Na2CO3/100kg water? (assume that 3% of the totalsolution is lost by evaporation)
Perfluorocarbons (PFCs), hydrocarbons with all the H re-placed by F, have very weak cohesive forces. One unusual appli-cation shows a mouse surviving submerged in O₂-saturated PFCs. (a) At 298 K, perfluorohexane (C₆F₁₄, M=338 g/mol,d=1.674 g/mL) in equilibrium with 101,325 Pa of O₂ has a mole fraction of O₂ of 4.28X10⁻³. What is the kH in mol/Latm?(b) According to one source, the kH for O₂ in water at 25°C is 756.7 L atm/mol. What is the solubility of O₂- in water at 25°C in ppm? (c) Rank the kH values in descending order for O₂- in water,ethanol, C₆F₁₄, and C₆H₁₄. Explain your ranking.
Acetonitrile, CH3CN, has a vapor pressure of 88.8 torr at 25.0 ̊C. If 9.22 mL of liquid acetonitrile (MCH3CN = 41.05 g/mol, dCH3CN = 0.786 g/mL) is placed into a sealed 5.25 L container at 25.0 ̊C and allowed to reach equilibrium. What would the value of [grams of CH3CN(g)/ grams of CH3CN(l)] in the container be at equilibrium?.
1.Calculate the normality of the solutions containing 5.267g/L K2Cr2O7 (the Cr is reduced to Cr3+).(FW=294.19 g/mol) 2.A and B react as follows: A + B 2C. The equilibrium constant is 5.0 x 106. If 0.40 mol of Aand 0.70 mol of B are mixed in 1L, what are the concentrations of A, B and C after reaction? 3. The following data is given at a certain temperature:(1) 2N2 (g) + O2 (g) 2N2O (g) K1 = 1.2 x 10-35(2) N2O4 (g) 2NO2 (g) K2 = 4.6 x 10-3(3) ½N2 (g) + O2 (g) NO2 (g) K3 = 4.1 x 10-9Calculate the molar equilibrium constant, K for the reaction:2N2O (g) + 3O2 (g) 2N2O4 (g)
The maximum solid solubility of carbon in ferrite occurs at 0.022 wt% C and 727 ° C, the eutectoid composition is 0.76 wt% C, the maximum solid solubility of carbon in austenite occurs at 2.14 wt% C and 1147 ° C, and the cementite composition is 6.7 wt% C. For 2122 g of a 3.2134 wt% C steel at 726 ° C, what will be the mass of carbon present as part of a compound?(a) 67.9 g(b) 74.2 g(c) 58.7 g(d) 83.5 g
A 19.51 ݃ sample of impure methylamine, which contains 72.58% (by mass) of CH3NH2 , isreacted with 30.81 ݃ of pure oxygen gas:4CHଷNHଶ(g) + 9Oଶ(g) ⟶ 4COଶ(g) + 10HଶO(ℓ) + 2Nଶ(g) In another experiment, this impure methylamine was used as follows: An unknown mass of the impure compound is dissolved in enough water to make 500.0 ݉ܮof solution. 20 ݉ܮ of this solution was transferred by pipette to a clean 250 mL volumetric flask andmade up to the mark. The molarity of the CH3NH2 in the final solution was determined to be 0.103 M.Determine the mass of CH3NH2 present in the original amount of impure compound used tomake this solution.
What mass of silver nitrate will precipitate out of solution if 950.0g of silver nitrate is initially dissolved into 225 g of water at 50oC and then the solution is cooled to 20oC?
The solubility of KNO3 (in gr KNO3 per 100 gr water) is 155 gr KNO3 at 75 oC and 38 gr KNO3 at 25 oC. What mass of KNO3 (in grams) will crystallize out of solution if exactly 100 gr of its saturated solution at 75 oC are cooled to 25 oC? a. 75.4 gr b. 30.7 gr c. 110 gr d. 45.9 gr
7.) At the surface of the earth, partial pressure of nitrogen gas is 0.78 atm. At normal body temp (37°C), the solubility of N2 gas (MW 28.01 g/mol) in water is 0.015 g/L. What is the solubility of N2 in blood (especially an aqueous solution) at a depth of 100 ft, where partial pressure of N2 is 3.12 atm. Express answer in g/L