What is the partial pressure of CO₂ at 468.2 K in a 25.0 L fuel combustion vessel if it contains 67.8 grams CO2, 82.1 g H₂O, and 7.30 mol vaporized, yet uncombusted fuel?
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- What is the partial pressure of CO₂ at 468.2 K in a 25.0 L fuel combustion vessel if it contains 61.8 grams CO₂, 82.1 g H₂O, and 7.30 mol vaporized, yet uncombusted fuel?What is the partial pressure (in atm) of CO₂ at 468.2 K in a 25.0 L fuel combustion vessel if it contains 60.0 grams CO₂, 82.1 g H₂O, and 7.30 mol vaporized, yet uncombusted fuel?Sulfur dioxide reacts with oxygen in the presence of plati- num to give sulfur trioxide: 2 SO2(g) + O2(g) → 2 SO3(g) Suppose that at one stage in the reaction, 26.0 mol SO2, 83.0 mol O2, and 17.0 mol SO3 are present in the reaction vessel at a total pressure of 0.950 atm. Calculate the mole fraction of SO3 and its partial pressure.
- While ethanol CH3CH2OH is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene CH2CH2 with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 200.mL flask with 1.2atm of ethylene gas and 1.3atm of water vapor. When the mixture has come to equilibrium she determines that it contains 0.25atm of ethylene gas and 0.35atm of water vapor. The engineer then adds another 0.30atm of ethylene, and allows the mixture to come to equilibrium again. Calculate the pressure of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits.(a) A rigid tank contains 1.60 moles of helium, which can be treated as an ideal gas, at a pressure of 28.0 atm. While the tank and gas maintain a constant volume and temperature, a number of moles are removed from the tank, reducing the pressure to 5.00 atm. How many moles are removed? mol (b) What If? In a separate experiment beginning from the same initial conditions, including a temperature T, of 25.0°C, half the number of moles found in part (a) are withdrawn while the temperature is allowed to vary and the pressure undergoes the same change from 28.0 atm to 5.00 atm. What is the final temperature (in °C) of the gas? °CIf 14.5g of calcium carbonate decomposes via the following reaction, how many liters of carbon dioxide at a temperature of 303K and 1.02atm will be produced? CaCO3(s)−→−heatCaO(s)+CO2(g) Use R=0.08206L atmmol K for the ideal gas constant. Your answer should have three significant figures.
- A steel cylinder contains 5.00 moles graphite (pure carbon) and 5.00 moles O2. The mixture is ignited and all the graphite reacts. Combustion produces a mixture of CO gas and CO2 gas. After the cylinder has cooled to its original temperature, it is found that the pressure of the cylinder has increased by 25.0%. Calculate the mole fractions of CO, CO2, and O2 in the final gaseous mixture. Mole fraction of CO = Mole fraction of CO2 = Mole fraction of O2 =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.Natural gas is a mixture of hydrocarbons, primarily methane (CH4) and ethane (C2H6). A typical mixture might have mole fraction of methane = 0.915 and mole fraction of ethane = 0.085. (a) What are the partial pressure of the two gases in a 14.10 L container of natural gas at 30 degrees Celcius and 1.34 atm? (b) Assuming complete combustion of both gases in the natural gas sample, what is the total mass of water formed? Hint: Write the balanced combustion chemical equation for each gas separately in the gas mixture to find the mass of water formed.
- 4. Answer the following question regarding mixtures of ideal gases: Find the total pressure (in atm) of a binary mixture of water vapor, H,O, with chlorine gas, Cl2. The partial pressure of chlorine gas is 134.63 psi, the partial pressure of water vapor is 525.8 torr. The volume is 70.9 L, temperature is 363.15 K, and the cylinder contains 21.79 moles Cl2.References Use the References to access important values if needed for this question. Zinc metal reacts with excess hydrochloric acid to produce hydrogen gas according to the following equation: Zn(s) + 2HCI(aq) ZnCl2(aq) + H2(g) The product gas, H2, is collected over water at a temperature of 25 °C and a pressure of 754 mm Hg. If the wet H2 gas formed occupies a volume of 6.46 L, the number of moles of Zn reacted was mol. The vapor pressure of water is 23.8 mm Hg at 25 °C. Submit AnswerThe pressure P of a sample of oxygen gas that is compressed at a constant temperature is related to the volume V of gas by a reciprocal function of the form P = k V . (a) A sample of oxygen gas that occupies 0.674 m3 exerts a pressure of 39 kPa at a temperature of 293 K (absolute temperature measured on the Kelvin scale). Find the value of k (in kPa · m3) in the given model.