A student wants to burn a 1.25 mL sample of ethanol (C2H5OH, d = 0.789 g/mL) in a jar containing dry air. The air in the jar is at standard atmospheric pressure and a temperature of 22 °C. Use this information and the composition of dry air in the previous problem to answer the following questions. a)Write a balanced chemical reaction for the combustion of ethanol. b)Calculate the moles of oxygen needed to completely combust the ethanol. c)Calculate the partial pressure of oxygen in the jar. d)Calculate the volume of oxygen (in L) needed in the jar.
A student wants to burn a 1.25 mL sample of ethanol (C2H5OH, d = 0.789 g/mL) in a jar containing dry air. The air in the jar is at standard atmospheric pressure and a temperature of 22 °C. Use this information and the composition of dry air in the previous problem to answer the following questions. a)Write a balanced chemical reaction for the combustion of ethanol. b)Calculate the moles of oxygen needed to completely combust the ethanol. c)Calculate the partial pressure of oxygen in the jar. d)Calculate the volume of oxygen (in L) needed in the jar.
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter10: Gases And Their Properties
Section: Chapter Questions
Problem 106IL
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A student wants to burn a 1.25 mL sample of ethanol (C2H5OH, d = 0.789 g/mL) in a jar containing dry air. The air in the jar is at standard atmospheric pressure and a temperature of 22 °C. Use this information and the composition of dry air in the previous problem to answer the following questions.
a)Write a balanced
b)Calculate the moles of oxygen needed to completely combust the ethanol.
c)Calculate the partial pressure of oxygen in the jar.
d)Calculate the volume of oxygen (in L) needed in the jar.
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