1.Amixture composed of CO and H2 is contained at 1/1 kPa. Calculate the partial pressure of the H2 in kPa in this mixture if the mole fraction of CO s 63%(3significant fig)
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Q: A student performed the experiment described in this module, using 4.00 mL of a 3.5% H2O2 solution…
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Q: What is the temperature in K of 0.795 mole of neon in a 2.00 L vessel at 4.32 bar? R = 0.08314…
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Q: What is the temperature in K of 0.500 mole of neon in a 2.0O L vessel at 4.32 bar? R = 0.08314 L·…
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- Unit 3: Barium bromate, Ba(BrO3)2, has a solubility product of 2.43 x 10-4 at STP. How many moles of barium bromate will dissolve per liter of water at STP?A certain gas mixture is at a pressure of 3500 kPa and is composed of 18.0 g of O2 and 28.0 g of CO2. Calculate the mole fraction of O2 gas in the mixture.The mole fraction of neon in dry air near sea level is 0.00001818, where the molar mass of neon is 20.183. The partial pressure of neon when the total atmospheric pressure (dry air) is 97.5 kPa is_____ kPa.
- A gas mixture at room temperature contains 10.0 mol CO and 12.5 mol 0,. (a) Compute the mole fraction of CO in the mixture. (b) The mixture is then heated, and the CÓ starts to react with the O, to give CO2: CO(g) + O2(g) –→ CO2(g) At a certain point in the heating, 3.0 mol CO, is present. Determine the mole fraction of CO in the new mixture.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?Explain in terms of the Kinetic Molecular Theory the following situations: a) Why does compressing a gas raise the temperature of the system? b) Explain why the density of a gas is so much lower than the density of its liquid form? c) Explain in detail the dissolving process of KCl in water. d) Explain why the solid precipitate AGl (s) forms when solutions of KCl (aq) and AgNO3 (aq) are mixed.
- A 1.52 g mixture of sucrose (CH,0, 342.30 g mol") and ethyl alcohol (C,H,O, 46.07 g mol") is reacted with acidic aqueous potassium dichromate (K,Cr,0,) solution. Produced 3.12 L CO, (g) is collected over water at 35 °C and has a barometric pressure of 0.52 atm. Water has a vapor pressure of 42.20 mmHg. Calculate the mass percent of C,H,O, in the mixture. CHOlaq) + Cr,O, (aq) - CO.(g) + Cr"(aq) (not balanced) CH.O(aq) + Cr,0, (aq) - CO.(g) + Cr" (aq) (not balanced) Enter only integer number, do not use % sign, Le. 12.345% should be entered as 12. Answer:A weighed quantity of PCI5(s) is sealed in a 100.0-cm³ glass bulb to which a pressure gauge is attached. The bulb is heated to 250°C, and the gauge shows that the pressure in the bulb rises to 0.895 atm. At this temperature, the solid PCI, is all vaporized and also partially dissociated into Cl2(g) and PCI3(g) according to the equation PCI5(g) 2 PCI3(g) + Cl(g) At 250°C, K = 2.15 for this reaction. Assume that the contents of the bulb are at equilibrium and calculate the partial pressure of the three different chemical species in the vessel.A student performed the experiment described in this module, using 6.00 mL of a 3% H2O2 solution with a density of 1.03 g mL-1. The water temperature was 22 ° C, and the barometric pressure in the laboratory was 30.30 in. Hg. After the student immersed the yeast in the peroxide solution, she collected 65.40 mL of Oz. (7) Calculate the mass of H2O2 in 5.00 mL of the H2O2 solution.
- Sulfur dioxide emissions from coal-based power plants areremoved by flue-gas desulfurization.The flue gas passes through a scrubber, and a slurry of wet calcium carbonate reacts with it toform carbon dioxide and calcium sulfite. The calcium sulfite then reacts with oxygen to form calcium sulfate, which is sold as gypsum. (a) If the sulfur dioxide concentration is 1000 times higher than its mole fraction in clean dry air (21010), how much calcium sulfate (kg) can be made from scrubbing 4 GL of flue gas (1 GL1X10^9L)? A state-of-the-art scrubber removes at least 95% of the sulfur dioxide. (b) If the mole fraction of oxy-gen in air is 0.209, what volume (L) of air at 1.00 atm and 25°C is needed to react with all the calcium sulfite?6-25. A mixture of gases contains 66.0 g CO2, 2.02 g of H₂, and 16.0 g of O₂. If the total pressure of the mixture is 725 torr, what is the partial pressure of each gas? 6-26. Air, by weight, is essentially a mixture of 79% N₂ and 21% O₂. Calculate the partial pressure of each gas at a total pressure of 99 kPakPa.A gas mixture contains 4.5 mol Br, and 33.1 mol F,. (a) Compute the mole fraction of Br, in the mixture. (b) The mixture is heated above 150°C and starts to react to give BrFs: Br2(g) + 5 F2(g) –→ 2 BrF;(g) At a certain point in the reaction, 2.2 mol BrF5 is present. Determine the mole fraction of Br2 in the mixture at that point.