When heated, NaOH decomposes according to the following equation. If all of the water is produced as water vapor, what is the expected mass loss for a 7.95 gram sample of NaOH? Report your answer with three significant figures.
2 NaOH (s) → Na2O (s) + H2O (g)
Solution : As we know that
No. Of moles = mass /molar mass
Therefore
No. Of moles of NaOH = 7.95 g/ 40g mol-1
= 0.198 mol
Now
Given reaction is
2 NaOH (s) Na2O (s) +H2O (g)
From the reaction we see that
2 mol of NaOH gives 1 mol of H2O
Therefore
No. Of moles of H2O =1/2 * No. Of moles of NaOH
No. Of moles of H2O = 0.198/2
= 0.099 mol
Therefore
Mass of H2O formed = 0.099 mol * 18.0 g mol-1
= 1.78 g
Thus
Mass of NaOH loss = mass of H2O formed
=1.78 g
When heated, NaOH decomposes according to the following equation. If all of the water is produced...
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