Explanation Given: The mole ratio of carbon monoxide and oxygen gas is 2.0 : 1.0 . The volume is 2.45 L , the pressure is 745 Torr , and the temperature is 552 ∘ C . The final pressure is 552 Torr . Explanation: The concerned reaction is as follows: 2CO ( g ) + O 2 ( g ) → CO 2 ( g ) Before the reaction, the pressure in atm is as follows: P 1 = 745 Torr × 1 atm 760 Torr = 0.980 atm The temperature in Kelvin is as follows: T ( K ) = 273 + T ( ∘ C ) = 273 + 552 ∘ C = 825 K Calculate the number of moles ( n 1 ) as follows: n 1 = P 1 V R T = 0.980 atm × 2.45 L 0.08206 L atm mol − 1 K − 1 × 825 K = 0.0355 mol After the reaction, the pressure in atm is as follows: P 2 = 552 Torr × 1 atm 760 Torr = 0.726 atm Calculate the number of moles ( n 2 ) present after the reaction as follows: n 2 = P 2 V R T = 0.726 atm × 2.45 L 0.08206 L atm mol − 1 K − 1 × 825 K = 0.0263 mol Assume the initial moles of CO as x and that of O 2 as y

Mastering Chemistry with Pearson eText -- Standalone Access Card -- for Chemistry: A Molecular Approach (4th Edition)

4th Edition

ISBN: 9780134162485

Author: Nivaldo J. Tro

Publisher: PEARSON

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Chapter 5, Problem 117E

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To determine: Percentage of carbon monoxide converted to carbon dioxide.

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Chapter 5, Problem 116E

Chapter 5, Problem 118E

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