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Ideal gas equation is PV=nRT where, P=pressure V=volume n=number of moles R=Gas constant T=temperatureGiven that V=4.40 LP=747 mmHgT=308KR=62.36 L mmHg/molKn=PVRTn=747mmHg×4.40L62.36mmHg/molK×308Kn=0.1711 mol 0.1711 moles of O2 are produced. According to the balanced chemical equation, 1 mole of O2 is produced from 2moles of Ag2O i.e. Ag2O is double the amount of O2. So, 0.1711 mole of O2 will be produced from 0.3422 moles of Ag2O. Molar mass of Ag2O= 231.735 g/mol Hence, mass of required Ag2O =moles ×molar mass=0.3422 moles×231.735 g/mol= 39.65 grams Answer=39.65 grams of Ag2O

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MReview | Constants . In the reaction shown here, 4.40 L of O2 was formed at P = 747 mmHg and T = 308 K. 2Ag0(s)-4Ag(s) + O2(9) Part A You may want to reference (Pages 444 - 446) Section 10.10 while completing this problem. How many grams of Ag,0 decomposed? Express the mass to three significant figures and include the appropriate units.

MReview | Constants . In the reaction shown here, 4.40 L of O2 was formed at P = 747 mmHg and T = 308 K. 2Ag0(s)-4Ag(s) + O2(9) Part A You may want to reference (Pages 444 - 446) Section 10.10 while completing this problem. How many grams of Ag,0 decomposed? Express the mass to three significant figures and include the appropriate units.

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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