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When sodium carbonate reacts with hydrochloric acid, the carbonic acid that is formed...

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t521863 | Student, Grade 10 | (Level 1) Valedictorian

Posted September 1, 2013 at 11:57 PM via web

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When sodium carbonate reacts with hydrochloric acid, the carbonic acid that is formed immediately breaks down into carbon dioxide and water. What mass of sodium carbonate would have been originally present if 5.0 L of carbon dioxide was produced? NA2CO3--> 2NaCL + CO2+H2O

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llltkl | College Teacher | (Level 3) Valedictorian

Posted September 2, 2013 at 7:18 AM (Answer #1)

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When sodium carbonate reacts with hydrochloric acid, the carbonic acid that is formed immediately breaks down into carbon dioxide and water. What mass of sodium carbonate would have been originally present if 5.0 L of carbon dioxide was produced?

The balanced chemical equation for the reaction of sodium carbonate  and hydrochloric acid is:

`Na_2CO_3 +2HCl = 2NaCl + CO_2 (g)+H_2O`

From the stoichiometry of this reaction, it follows that:

At NTP, 1 gram-mole, i.e. 22.4 litre `CO_2 (g)` is produced from (2*23+12+3*16), i.e. 106 g `Na_2CO_3` .

Therefore 5.0 L `CO_2` (g) will be produced from `(106*5.0)/22.4=23.66` g `Na_2CO_3`

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ayl0124 | Student, Grade 12 | (Level 1) Valedictorian

Posted August 13, 2014 at 8:55 PM (Answer #2)

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Use stoichiometry to solve this problem. The units cross each other out, leaving you with "g Na2CO3."

`5.0"L(CO_2)" = (1"mol(CO_2)")/(22.4"L(CO_2)") = (1"mol(Na_2CO_3)")/(1"mol(CO_2)") = (105.99"g(Na_2CO_3)")/(1"mol(Na_2CO_3)") = 23.66"g(Na_2CO_3)" `

You would need 24 grams of Na2CO3 to produce 5.0 L of CO2. Note that you need two sig figs in your answer because you began with two sig figs. 

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