# chemistry

A method for scrubbing CO2(g) from the air on a spacecraft is to allow CO2(g) to react with NaOH according
to the following (unbalanced reaction).
NaOH(s) + CO2(g) → Na2CO3(s) + H2O(l)
Use the appropriate thermodynamic tables to calculate the enthalpy, entropy and standard Gibbs free energy
at 298K. (For the solid sodium carbonate, you need to use the following data: Molar heat capacity at constant
pressure 112.3 J/(mol K), Standard molar entropy 135 J/(mol K), Standard molar enthalpy of formation -1130.7
kJ/mol)
Any help to figure this out would be great I don't even know where to start

1. 2
1. The problem doesn't say so but implies you want the dH, dS, dG FOR THE REACTION.
1. You have the equation, balanced it.
2. dHrxn = (n*dHf products) - (n*dHf reactants)
3. dSrxn = (n*dSf procuts) - (n*dSf reactants)
4. Then dGrxn = dHrxn - TdSrxn. Substitute and solve for dG.
Post your work if you get stuck.

The dHf and dSf you will need for Na2CO3 is listed in the problem. I presume the others are listed in your text/notes.

posted by DrBob222

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