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

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter6: Thermochemistry

Section: Chapter Questions

Problem 130CP: Consider 2.00 moles of an ideal gas that are taken from state A (PA = 2.00 atm, vA = 10.0 L) to...

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Concept explainers

Thermochemistry

Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.

Exergonic Reaction

The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.

Question

B IU Av A
1. Using the Ideal Gas Law (PV = nRT), calculate the grams of O2 produced in the reaction. Show
%3D
your 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 of
oxygen gas.
e. Use the moles of oxygen gas found and the molar mass of O2 to calculate the grams of
oxygen produced using dimensional analysis.

Table 2: Temperature, Pressure, and Volume Data
Room (or
regional)
Pressure
Final Volume
Volume of O2
Temperatur
e of Tap
Water (°C)
Initial
Volume
of Air (mL)
of Air
Collected
(after
reaction) (mL)
(Final Volume-
Initial Volume)
(atm)
37
1 atm
10mL
50mL
40mL
Table 3: Reaction Time Data
Time Reaction
Time Reaction
Ended
Total Reaction Time
Started
3:30
3:33
3 min

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