B IU Av A1. Using the Ideal Gas Law (PV = nRT), calculate the grams of O2 produced in the reaction. Show%3Dyour work and follow the steps below.If you pressure is not yet in atm, convert it to atm using the appropriate conversion factor.b. Convert the volume of oxygen collected from mL to L.C.Convert the temperature of the water from °C to K.d. Plug in P, V, R (gas constant), and T to the ideal gas law and solve for n, which is moles ofoxygen gas.e. Use the moles of oxygen gas found and the molar mass of O2 to calculate the grams ofoxygen produced using dimensional analysis. Table 2: Temperature, Pressure, and Volume DataRoom (orregional)PressureFinal VolumeVolume of O2Temperature of TapWater (°C)InitialVolumeof Air (mL)of AirCollected(afterreaction) (mL)(Final Volume-Initial Volume)(atm)371 atm10mL50mL40mLTable 3: Reaction Time DataTime ReactionTime ReactionEndedTotal Reaction TimeStarted3:303:333 min

Given, Pressure = 1 atm Volume = 40 mL Temperature = 37°C

URI), calculate the grams of O2 produced in the reaction. S your work and follow the steps below. a. If you pressure is not yet in atm, convert it to atm using the appropriate conversion b. Convert the volume of oxygen collected from mL to L. C. Convert the temperature of the water from °C to K. d. Plug in P, V, R (gas constant), and T to the ideal gas law and solve for n, which is m oxygen gas.

URI), calculate the grams of O2 produced in the reaction. S your work and follow the steps below. a. If you pressure is not yet in atm, convert it to atm using the appropriate conversion b. Convert the volume of oxygen collected from mL to L. C. Convert the temperature of the water from °C to K. d. Plug in P, V, R (gas constant), and T to the ideal gas law and solve for n, which is m oxygen gas.

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter5: Gases

Section: Chapter Questions

Problem 5.110PAE

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