How Many Grams of CO2 Are Collected at 104.3 kPa and 29.6°C?

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SUMMARY

The discussion focuses on calculating the grams of carbon dioxide collected at a pressure of 104.3 kPa and a temperature of 29.6°C using the ideal gas law equation PV=nRT. The gas constant used is 0.08206 L·atm/mol·K. Participants highlighted the need to first determine the volume of CO2 at standard temperature and pressure (STP) before applying the ideal gas law to find the mass at the specified conditions. The solution involves understanding the relationship between the molecular formula of the hydrocarbon and the combustion reaction to derive the amount of CO2 produced.

PREREQUISITES
  • Understanding of the Ideal Gas Law (PV=nRT)
  • Knowledge of standard temperature and pressure (STP)
  • Familiarity with stoichiometry in chemical reactions
  • Basic skills in converting between liters and grams
NEXT STEPS
  • Learn how to apply the Ideal Gas Law in various conditions
  • Study the concept of molar volume at STP
  • Explore stoichiometric calculations in combustion reactions
  • Investigate the properties of carbon dioxide and its behavior under different pressures and temperatures
USEFUL FOR

Chemistry students, educators, and anyone involved in gas law calculations or combustion analysis will benefit from this discussion.

Korupt
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Homework Statement


If carbon dioxide is collected at 104.3 kPa and 29.6 oC, how many grams are collected? Use the gas constant of 0.08206 L. atm/mol . K.

1. Liters at STP.
2. Grams at new temperature and pressure.

Homework Equations


PV=nRT


The Attempt at a Solution


I really don't understand what the problem wants me to do, there's not enough info to use PV=nRT equation and I don't know any other ideal gas ones except for the Combined Gas Law Equation which is also not applicable. Perhaps it has something to do with the earlier part of the problem which is all here: http://www.duluthhigh.org/tpindexy.php?page=myhome&id=104 but it doesn't seem to. I solved 1-5 but with 6 and 7 I really have no clue and this is a summer assignment so we really haven't learned anything yet. Any help is appreciated. Thanks.
 
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It sounds to me that it does depend on the previous questions. You found the molecular formula of the unknown hydrocarbon in question 2, and then are told that "53.21 L of the substance burns in 84.31 L of oxygen". You can write a chemical equation for the combustion and use the volumes of the limiting reagent to find how much carbon dioxide is produced.
 
Thanks, I was able to figure it out that way.
 

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