Calculating Pressure in the Stomach after Taking Tums

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Discussion Overview

The discussion revolves around calculating the pressure in the average adult stomach after taking Tums, focusing on the chemical reaction that produces gas and the application of the ideal gas law. The scope includes theoretical calculations and assumptions related to chemistry and physics.

Discussion Character

  • Homework-related
  • Mathematical reasoning

Main Points Raised

  • One participant suggests using the ideal gas law (PV=nRT) to calculate pressure, given the volume of the stomach and the reaction producing gas.
  • Another participant questions the weight of a Tums tablet and seeks clarification on the amount of CO2 produced from the reaction.
  • A participant calculates that two Tums tablets weigh 500 mg and proposes that this corresponds to approximately 0.0049 moles of CO2.
  • There is a discussion about body temperature, with one participant stating it as 37 degrees Celsius and converting it to Kelvin for use in the gas law equation.
  • Another participant confirms that all variables except pressure are known at this point.

Areas of Agreement / Disagreement

Participants generally agree on the approach to use the ideal gas law and the values for temperature and volume, but there is no consensus on the exact calculations or assumptions regarding the amount of CO2 produced.

Contextual Notes

There are unresolved assumptions regarding the complete reaction of Tums and the exact conditions in the stomach, which may affect the calculations.

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Homework Statement


Tums react in your stomach to produce a gas. The average adult stomach expand to one liter when full. Calculate the pressure in the average adult stomach after taking 2 Tums.

Homework Equations


Since its asking for pressure, and the volume is given perhaps PV=nRT should be used.
Also P1V1=P2V2 might seem like a possible equation.


The Attempt at a Solution


I'm honestly not sure how to start this problem. I started with a balanced chemical equation for the reaction of the Tums (CaCO3) and the stomach acid/hydrochloric acid (HCl), which would be:
CaCO3 + 2HCl --> CaCl2 + H2O + CO2. I'm not sure where to go from here or if this is a necessary step in solving the problem. Any suggestions in where to start would be helpful.
 
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What is the weight of a "tum"?
How much CO2 do you get from the reaction? (In any unit you like)
 
One tums tablet is 250 mg. So two tums tablets would be 500 mg or .5 grams. If so, then would .0049 moles of CO2 sound correct?
 
Last edited:
Yes.

What is a body temperature?
 
37 degrees Celsius. Converted to kelvins it would be 310.15 K. Would I use this as the temperature in the equation PV=nRT?
 
Sure. I think everything apart from pressure is known now.
 

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