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pelow, what would be the final pressure of carbon ming it had the full 2.00 L in which to expand? )→ H:O(1) + CO:(g)

pelow, what would be the final pressure of carbon ming it had the full 2.00 L in which to expand? )→ H:O(1) + CO:(g)

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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**Problem: Calculating the Final Pressure of Carbon Dioxide** If 65.4 grams of carbonic acid are sealed in a 2.00 L soda bottle at room temperature (298.15 K) and decompose completely via the equation below, what would be the final pressure of carbon dioxide (in atm) assuming it had the full 2.00 L in which to expand? \[ \text{H}_2\text{CO}_3(\text{aq}) \rightarrow \text{H}_2\text{O}(\ell) + \text{CO}_2(\text{g}) \]
Transcribed Image Text:**Problem: Calculating the Final Pressure of Carbon Dioxide** If 65.4 grams of carbonic acid are sealed in a 2.00 L soda bottle at room temperature (298.15 K) and decompose completely via the equation below, what would be the final pressure of carbon dioxide (in atm) assuming it had the full 2.00 L in which to expand? \[ \text{H}_2\text{CO}_3(\text{aq}) \rightarrow \text{H}_2\text{O}(\ell) + \text{CO}_2(\text{g}) \]
Expert Solution
Step 1

Mass of H2CO3 = 65.4 g

Molar mass(MM) of H2CO3 = 62 g

Moles = mass/MM

     = 65.4/62 = 1.06 mol

From balanced reaction, 

1 mol H2CO3 = 1 mol CO2

1.06 mol H2CO3 = 1.06 mol CO2 

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