[maturak159]

Hi there,

My questions are in relation to the following system:

NaOH(s) <> Na (aq) + OH (aq) + energy

When NaCl (or just Na) is added:
 i) Does the equilibrium shift to the left still despite the reactants being a solid?
 ii) Does the concentration of OH reduce as a result of the equilibrium shifting to the left even though it isn't technically being consumed to form anything (as NaOH is solid)?

Thanks in advance.

[AWK]

NaOH(s) <> Na (aq) + OH (aq) + energy

NaOH(s) = Na(aq)⁺ + OH(aq)^-
This process is practically irreversible

Take better example for equilibrium discussion.

[maturak159]

I suppose a better example could be:

S(s) + O2(g) <> SO2(g) + energy

What you are saying though is that it is very unlikely for there to be a single reactant which is a solid? Hence the questions asked are invalid?

[AWK]

Solid sulfur does not undergo combustion directly. You can burn vapours over liquid sulfur. Flash point for sulfur is 207 C (boiling point 444.6 C). Of course, for energy calculation we often use standard conditions, but this is recalculation of energy to 25 C, not real reaction conditions.