At standard temp and pressure (which is sea level pressure of about 1 atm and25°C) we can assume the following relationship- 24,000 mL of gas = 1 mole ofgas molecules. In fermentation, we can also assume that the ratio of gas%3Dmolecules and ATP are equal to each other, ie 1 mole of gas = 1 mole of ATP.%3DIf we were to produce 12.0 mL of gas in a fermentation reaction, how manymoles of ATP will we have produced in the fermentation process?

Given, At 1 atm pressure and 25°C temperature, 24000mL of gas = 1 mole of gas molecules And, 1 mole…

At standard temp and pressure (which is sea level pressure of about 1 atm and 25°C) we can assume the following relationship- 24,000 mL of gas = 1 mole of gas molecules. In fermentation, we can also assume that the ratio of gas molecules and ATP are equal to each other, ie 1 mole of gas = 1 mole of ATP. %3! If we were to produce 12.0 mL of gas in a fermentation reaction, how many moles of ATP will we have produced in the fermentation process?

At standard temp and pressure (which is sea level pressure of about 1 atm and 25°C) we can assume the following relationship- 24,000 mL of gas = 1 mole of gas molecules. In fermentation, we can also assume that the ratio of gas molecules and ATP are equal to each other, ie 1 mole of gas = 1 mole of ATP. %3! If we were to produce 12.0 mL of gas in a fermentation reaction, how many moles of ATP will we have produced in the fermentation process?

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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