[DeKeith]

Mass of whole tablet = 3.478 g
Mass of 1/2 tablet taken for reaction = 1.973
Volume of CO2 + water vapor ( corrected ) = 314 mL
Temperate of gas = 22.0 C
Vapor pressure at 22.0 C = 21 torr
Corrected Barometric pressure  = 757 torr


I need to solve for:


1. Partial pressure of CO2

2. Moles of Co2

3. Moles of NaHCO3

4. Mass of NaHCO3

5. Mass % in NaHCO3 in alka seltzer

6. mg of NAHCO3 per one tablet



My assumption is that the mole ratio of CO2 to NaHCO3 is 1:1. So would i just plug in my data into the ideal gas law and solve for the moles of CO2 first, then use that mole value to solve for the partial pressure of CO2? I'm just confused here. Any help?

[Borek]

My assumption is that the mole ratio of CO2 to NaHCO3 is 1:1.

Correct.

So would i just plug in my data into the ideal gas law and solve for the moles of CO2 first, then use that mole value to solve for the partial pressure of CO2?

Quite the opposite - you should find partial pressure of CO₂ and use it to find number of moles of CO₂ using ideal gas law.

Hint: you have collected gas over water? What is the collected gas total pressure? What gasses partial pressures are summed up in the collected gas?