Acidification of sodium bicarbonate (NaHCO3) produces carbon dioxide in a two step process.
The first step produces carbonic acid (H2CO3). Write and balance the molecular equation for the first step of the reaction of sodium bicarbonate with HClO4. (Do not include symbols for state of matter in your answer).
The second step is the decomposition of carbonic acid to carbon dioxide. Write and balance the molecular equation for the second step.
Now write the overall net ionic equation for the acidification of NaHCO3 to produce CO2.
What is the molar ratio of CO2 produced to NaHCO3 decomposed?
What mass of CO2 will be produced by the complete decomposition of 1156 mg of NaHCO3?
Thank you for any help.
2007-09-27 06:14:49 · 1 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
To the answer below. Everything was correct except for the third part. The overall Ionic equation.
2007-09-27 07:12:40 · update #1
NaHCO3 + HClO4 ===> H2CO3 + NaCLO4
H2CO3 ===> CO2 + H2O
H+ + HCO3- ===> CO2 + H2O
1/1
Atomic weights: Na=23 H=1 C=12 O=16 NaHCO3=84 CO2=44 Millimole=mmol
1156mgNaHCO3 x 1mmolNaHCO3/84mgNaHCO3 x 1mmolCO2/1mmolNaHCO3 x 44mgCO2/1molCO2 = 605.5mg CO2
2007-09-27 07:03:39 · answer #1 · answered by steve_geo1 7 · 0⤊ 0⤋