The stopcock connecting a 2.73 L bulb containing nitrogen gas at a pressure of 3.93 atm, and a 6.63 L bulb containing krypton gas at a pressure of 1.04 atm, is opened and the gases are allowed to mix. Assuming that the temperature remains constant, the final pressure in the system is __________ atm.

The stopcock connecting a 2.73 L bulb containing nitrogen gas at a pressure of 3.93 atm, and a 6.63 L bulb containing krypton gas at a pressure of 1.04 atm, is opened and the gases are allowed to mix. Assuming that the temperature remains constant, the final pressure in the system is __________ atm.

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter8: Gases

Section: Chapter Questions

Problem 155CP: Methane (CH4) gas flows into a combustion chamber at a rate of 200. L/min at 1.50 atm and ambient...

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Methane (CH4) gas flows into a combustion chamber at a rate of 200. L/min at 1.50 atm and ambient temperature. Air is added to the chamber at 1.00 atm and the same temperature, and the gases are ignited. a. To ensure complete combustion of CH4 to CO2(g) and H2O(g), three times as much oxygen as is necessary is reacted. Assuming air is 21 mole percent O2 and 79 mole percent N2, calculate the flow rate of air necessary to deliver the required amount of oxygen. b. Under the conditions in part a, combustion of methane was not complete as a mixture of CO2(g) and CO(g) was produced. It was determined that 95.0% of the carbon in the exhaust gas was present in CO2. The remainder was present as carbon in CO. Calculate the composition of the exhaust gas in terms of mole fraction of CO, CO2, O2, N2, and H2O. Assume CH4 is completely reacted and N2 is unreacted.
Consider a box divided in half. One side is filled with 1 mol Ne at 300 Kelvin, and the other is filled with 1 mol Rn at 300 Kelvin. A small hole is opened in the divider between the sides, allowing the gases to mix. Suppose it takes 4.0 minutes for the Rn pressure to equilibrate between the two sides. How long (min) will it take the Ne pressure to equilibrate?
At 27 °C, 500 cc of H2, measured under a pressure 400 torr, and 1000 cc of N2, measured under a pressure of 600 mm Hg, are introduced into an evacuated 2-L flask. Calculate the resulting pressure. (Given -> Unknown -> Solution -> Answer)
A gas occupies 50.0mL at 90.0 kpa. Find the volume at 135 kpa.
A syringe with friction free plunger has a pressure of one atmosphere acting down on plunger, 47 C, 1.60 x 10-3 mole, 40.0 mL. if add 1/4 more molecules while temperature is constant, what are the new T, P, and V?
we use Pv=nRT. Everything here should be related to H2 (g) --> Chemical equation1Mg +2 HCl à MgCl2 +H2(g) From video : mass of Mg =.0407 g H2 gas volume = 38.2ml Temperature of room=24.0 +273=297k Total Pressure of the room = 30.01 in mmHg Calculations: find total pressure from barometer and convert it to mmHg, 1 in =2.54 cm and 25.4 mm 30.01 in mmHg x 25.4 mm Hg =762.3 mmHg total pressure of room 1in mmHg First step- convert g of Mg to mol of H2 0.0407g Mg x 1mol/24 gx 1molH2 = 0.00169mol 1mol Mg Second step: Total pressure of gas = Pressure of H2 + P of water 762.3 = p H2 + 22.4 FROM reference (canvas)=Pressure of water at 24 C= 22.4 mmHg n= 0.00169mol H2 Pressure of H2= 762.3-22.4= 739.854 x 1atm/760= 0.973 atm H2 Volume of H2= 38.2 ml /1000 =0.038L H2 Temp= 297K anwer this quesions with the information provide: Using PV=nRT, Find R=? (No R averge needed) à 0.973X0.0382=0.00169XRx 297 0.0372=0.50R Then, Percent error…
A car generates 5000 L of exhaust at 450. °C and 0.1 atm. How many mol of exhaust gas is this? Write out the problem on paper in order to answer the questions related to the setup and the calculation for this problem. Rearrange the gas law equation to solve for the variable of interest. Identify which terms are in the numerator and which terms are in the denominator after rearranging. Do not leave any blank empty. Enter a zero "0" if the blank is not needed. Use the following abbreviations: pressure = P; volume = V, moles = n, gas constant = R, temperature = T Terms in the numerator: , , Terms in the denominator: , , What temperature (with proper s.f.) is entered into the equation? Enter the value in the first blank and the units in the second blank. Calculate the answer and use the two blanks to report with value (decimal notation, including proper s.f.) and units.
Let's call the initial temperature T1 = 290 K, and so the initial pressure is P1 = 1.80 ✕ 106 Pa. The final temperature is then T2 = 330 K. Calculate the final pressure. (Reminder—use the letter "e" to express scientific notation in your response. For example, if your answer is 1.2 ✕ 104, enter it as 1.2e4.) P2 = _________ Pa Let's try another example. Suppose we now have a gas initially at a pressure of 1.30 ✕ 106 Pa and a temperature of 400 K. The gas is in a cylinder with an adjustable piston sealing it in. We then reduce the volume of the container to one-third 1 3 of its original value, but maintain a constant pressure of 1.30 ✕ 106 Pa. What is the new final temperature (in K) of the gas? _______ K
Gaseous ammonia is injected into the exhaust stream of a coalburning power plant to reduce the pollutant NO to N2 according to the reaction:4 NH3( g) + 4 NO( g) + O2( g)----> 4 N2( g) + 6 H2O( g)Suppose that the exhaust stream of a power plant has a flow rate of 335 L/s at a temperature of 955 K, and that the exhaust contains a partial pressure of NO of 22.4 torr. What should be the flow rate of ammonia delivered at 755 torr and 298 K into the stream to react completely with the NO if the ammonia is 65.2% pure (by volume)?
For PV = nRT to be valid, the gas has to act______________
Consider Figure 13.1. If the height of the mercury column in the leveling bulb is 21 mm greater than that in the gas buret and atmospheric pressure is 600 mm , what is the pressure on the gas trapped in the buret? Should I assume (1 atm) or would I assume the atm is 600mm (standard) and subtract the 21 from the 600, then convert by division (600-21)/760 ?? thanks
Recorded barometric pressure: 758.9 mmHg Mass of Aluminum used= .021 g Volume of gas in gas burette after placing into leveling tank= 23 mL temperature in levelling tank: 21 oC Room Temperature: 294.45 K Partial pressure of water vapor: 17.5 mmHg 2 Al (s)+ 6HCl (aq)>>>>2 AlCl3 (aq)+ 3 H2 (g) 1. How to calculate the theoretical yield of H2 gas (mL) based on the mass of Aluminum used. 2. How to calculate the % error of H2 gas.