Question

In: Chemistry

If 1 grams of sodium bicarbonate are decomposed, determine the combined mass loss (in grams) of...

If 1 grams of sodium bicarbonate are decomposed, determine the combined mass loss (in grams) of water and carbon dioxide that are produced. When a 1.08g mixture of sodium chloride and sodium bicarbonate were heated for several minutes in a crucible and the mass after the first 3 heating intervals remained 0.8 grams.

What is the combined mass loss of water and carbon dioxide per gram on sodium bicarbonate?

Solutions

Expert Solution

Ans. 1. 2 NaHCO3(s) -----Heat---------> Na2CO3(s) + CO2(g) + H2O(g)

Moles of NaHCO3 = Mass/ Molar mass’

                                    = 1.000 g / (84.006908 g/ mol)

                                    = 0.011904 mol

According to the stoichiometry of balanced reaction, 2 mol NaHCO3 produces 1 mol each of CO2 and H2O.

So,

            Moles of H2O = moles of CO2 = (1/2) x Moles of NaHCO3

                                                            = (1/2) x 0.011904 mol

                                                            = 0.005952 mol

Now,

Total loss in mass = Mass of 0.005952 mol CO2 + Mass of 0.005952 mol H2O

                        = (0.005952 mol x 44.0098 g mol-1) + (0.005952 mol x 18.01528g mol-1)

                        = 0.261942 g + 0.107225 g

                        = 0.369167 g

#2. # Loss in mass after 4th drying = Initial mass of sample – Dried mass of sample

= 1.08 g – 0.8 g

= 0.28 g

# Calculate Moles of NaHCO3 in sample:

H2O and CO2 are lost as gases. So, net loss in mass during drying must be equal to the mass lost in form of H2O and CO2.

See the stoichiometry of decomposition, 2 mol NaHCO3 produces releases 1 mol each of CO2 and H2O.

Let the number of moles of NaHCO3 in the mixture be X.

So,

Moles of H2O lost = 0.5X

Moles of CO2 lost = 0.5X

Now,

Mass of H2O lost = Moles x Molar mass = 0.5X mol x (18.01 g/mol) = 9.005X g

Mass of CO2 lost = 0.5X x (44.01 g/mol) = 22.005X g

Total mass lost in form of H2O and CO2 = 9.005X + 22.005X = 31.010X g

So, 31.010X g must be equal to 0.28 g – the mass lost during drying.

Or, 31.010X g = 0.28 g

Or, X = 0.28 / 31.010 = 0.009029

Hence, X = 0.009029

Therefore, moles of NaHCO3 in sample = X moles = 0.009029 mol

# Calculate mass of NaHCO3 in original sample:

Mass of NaHCO3 in sample = Moles of NaHCO3 x Molar mass

= 0.009029 mol x (84.006908 g/mol)

= 0.7585 g

# Combined mass lost = 0.28 g

Mass of NaHCO3 in sample = 0.7585 g

Now,

Combined mass loss per g Na-bicarbonate = Combined mass loss / Mass of NaHCO3

                                                = 0.28 g mass loss / 0.7585 g NaHCO3

                                                = 0.369 g CO2 and H2O per gram NaHCO3


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