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- How does hydraulic fracturing differ from previously used techniques for the recovery of natural gas from the earth?What possible uses exist for the natural gas liquids that are removed from natural gas during its processing?Each sketch below shows a flask with some gas and a pool of mercury in it. The gas is at a pressure of 0.5 atm. A J-shaped tube is connected to the bottom of the flask, and the mercury can freely flow in or out of this tube. (You can assume that there is so much more mercury in the pool than can fit into the tube that even if the J-tube is completely filled, the level of mercury in the pool won't change.) Notice also that in the left sketch the J-tube is open at its other end, so that air from the atmosphere can freely flow. On the other hand, in the right sketch the J-tube is closed at its other end, and you should assume there is no gas between the mercury and the closed end of the tube. To answer this question, you must decide what the mercury level will be when the mercury finally stops flowing in or out of the tube. By moving the sliders back and forth, you'll see different levels of mercury in the J-tube. Select the final correct level for each sketch. A open tube closed tube -…
- 6. If excess carbon is present in a container that originally has 1:1 of CO and CO2 and no other gases, please explain the change of CO:CO2 ratio with increasing temperature.Each sketch below shows a flask with some gas and a pool of mercury in it. The gas is at a pressure of 1 atm. A J-shaped tube is connected to the bottom of the flask, and the mercury can freely flow in or out of this tube. (You can assume that there is so much more mercury in the pool than can fit into the tube that even if the J-tube is completely filled, the level of mercury in the pool won't change.) Notice also that in the left sketch the J-tube is open at its other end, so that air from the atmosphere can freely flow. On the other hand, in the right sketch the J-tube is closed at its other end, and you should assume there is no gas between the mercury and the closed end of the tube. To answer this question, you must decide what the mercury level will be when the mercury finally stops flowing in or out of the tube. By moving the sliders back and forth, you'll see different levels of mercury in the J-tube. Select the final correct level for each sketch. 1 1 2 I Don't Know open tube…The decomposition of 30.354 g of potassium chlorate yields solid potassium chloride and oxygen gas that is collected at 27.05°C and a pressure of 1.075 atm. The value for the gas constant, R, is 0.08206 L•atm/mol•K. Write a balanced equation for the reaction. What volume of oxygen gas is collected in this decomposition reaction? What mass of potassium chlorate needs to decompose in order to produce 11.889 L of oxygen gas collected at the same temperature and pressure as the original experiment?
- Hydrogen gas is collected over water at 23.5 °C and an atmospheric pressure of 765 mmHg. Calculate the partial pressure of hydrogen gas.A 4.00 L flask contains 1.40 atm argon at 25°C. a) Calculate the moles of argon gas initially present in the flask. b) 20 mol Cl2 is added to the flask and the total pressure of gas changes. Explain the molecular-level reasons for this pressure change. c) Using your knowledge of gases and intermolecular forces, predict (and explain) whether the argon or the chlorine would behave more like an ideal gas.Given the following equation: Mg(s) + 2HCl(aq) --> MgCl2(aq) + H2(g) After the reaction was completed the dry hydrogen gas(dry hydrogen gas means that the water vapor pressure has already been subtracted) had a volume of 2.00L at a pressure of 4.50atm and a temperature of 35C. If excess HCl was used, how much Magnesium metal was consumed. The atomic mass of Mg is 24.31g/mol.
- A 5.00 L flask is evacuated and 44.81 g of solid dinitrogen tetroxide, N2O4, is introduced at −196 °C. The sample is then warmed to 25 °C during which time the N2O4 vaporizes and some of it dissociates to form brown NO2 gas. The pressure slowly increases until it stabilizes at 3.27 atm. 1. Write the balanced reaction for the dissociation of N2O4. 2. What would be the pressure in the flask at 25 °C if the gas were all N2O4? 3. What would be the pressure in the flask at 25 °C if all of the gas converted into NO2? 4. What are the mole fractions of N2O4 and NO2 once the pressure in the flask stabilizes at 3.27 atm?A 5.00 L flask is evacuated and 44.81 g of solid dinitrogen tetroxide, N2O4, is introduced at −196 °C. The sample is then warmed to 25 °C during which time the N2O4 vaporizes and some of it dissociates to form brown NO2 gas. The pressure slowly increases until it stabilizes at 3.27 atm. 1. Write the balanced reaction for the dissociation of N2O4. 2. What would be the pressure in the flask at 25 °C if the gas were all N2O4? 3. What would be the pressure in the flask at 25 °C if all of the gas converted into NO2? 4. What are the mole fractions of N2O4 and NO2 once the pressure in the flask stabilizes at 3.27 atm? If we could please work through Part 4, that would be great :)Consider a sample of a hydrocarbon (a compound consisting of only carbon and hydrogen) at 0.959 atm and 298 K. Upon combusting the entire sample in oxygen, you collect a mixture of gaseous carbon dioxide and water vapor at 0.755 atm and 375 K. This mixture has a density of 0.6955 g/L and occupies a volume eight times as large as that of the pure hydrocarbon under initial conditions. Determine the molecular formula of the hydrocarbon. (Enter the elements in the order: C, H.) Molecular formula: Submit Answer Try Another Version 3 item attempts remaining
