How many moles of CO2 are present in the flask after 4mL of HCl have been added? What is the stoichiometric ratio between HCl and CO2?

Question

Flask is 150 mL. P=1.81 atm. Gas volume=135.9 ml. Liquid volume=14.1mL.

Initial pressure = 1 atm and initial temperature is 21.5 C

 I need help with putting this into an equation and writing the balanced equation for sodium bicarbonate and HCl.

Answer 1

The balanced chemical equation for sodium bicarbonate being neutralized by hydrochloric acid is:

NaHCO₃ + HCl → CO₂ + H₂O + NaCl

So, to answer one of your questions, the stoichiometric ratio between HCl and CO₂ is 1:1.

To answer the rest of your questions, I need clarification.

1. Do we have enough sodium bicarbonate that it will not be the limiting reagent?
2. Is the initial pressure, before adding HCl, 1 atm, and the final pressure, after the reaction, 1.81 atm?
3. Is the final pressure due to carbon dioxide only, or does the problem note that the partial pressure of water also contributes to the total pressure?
4. You give an initial temperature. Is there a final temperature, or does the temperature remain constant?

Add these clarifications, or copy the problem word-for-word from your assignment, and I'd be happy to help you get through the rest of it.