Thermal decomposition of 2.968g of a mixture containing NaHCO3 lost 0.453g. Calculate the percentage of NaHCO3 in this unknown mixture.Calculate the percentage of NaHCO3 in this unknown mixture.?
thermal decomp of NaHCO3 occurs as follows
2NaHCO3 --------%26gt;Na2CO2(s) + H2O(g) + CO2(g)
CO2 and H2O are evolved as gases, so the mass lost is the mass of CO2 and H2O produced.
The balanced equation shows that H2O and CO2 are produced in a 1:1 ratio. So the 0.453 g lost represents equal moles of H2O and CO2
Thus let n = moles
n x molar mass H2O + n x molar mass CO2 = 0.453
18.016n + 44.01n = 0.453
62.026 n = 0.453
n = 0.453 / 62.026
= 0.007303 moles of H2O and CO2 are formed
2 moles NaHCO3 decomposes to form 1 mole of H2O
Therefore moles NaHCO3 = 2 x moles H2O
= 0.014607 mol NaHCO3
mass NaHCO3 = molar mass x moles
= 84.008 g/mol x 0.014607 mol
= 1.227 g
% mass = actual mass / total mass x 100/1
= 1.227 g / 2.968 g x 100/1
= 41.34 %
= 41.3 % (3 sig figs)
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