Question

Na2CO3 + CO2 + H2O → 2 NaHCO3 How many grams of soda ash would be needed to produce 1.00 kg of sodium hydrogen carbonate?

Answer 1

The first step we have to follow is to convert the given mass of sodium hydrogen carbonate to moles using its molecular mass (MM=84kg/kmol):

`1.00kgNaHCO_3\cdot(1kmolNaHCO_3)/(84kgNaHCO_3)=0.012kmolNaHCO_3`

Now, use the stoichiometric ratio given by the equation to find how many moles are needed to produce 0.012kmoles of NaHCO₃:

`0.012kgNaHCO_3\cdot(1kmolNa_2CO_3)/(2kmolNaHCO_3)=0.006kmolNa_2CO_3`

Now, convert the estimated amount of Na2CO3 to mass using its molecular mass (MM=106kg/kmol):

`0.006kmolNa_2CO_3\cdot(106gNa_2CO_3)/(kmolNa_2CO_3)=0.636kgNa_2CO_3`

Convert the mass in kg to g:

`0.636kgNa_2CO_3\cdot(1000gNa_2CO_3)/(1kgNa_2CO_3)=636gNa_2CO_3`

It means that the answer is 636g of soda ash are needed to produce 1.00 kg of sodium hydrogen carbonate.