11. Given the following reaction: 2 HCHOH (1) + 3 O (g) 4 CO (g)...

 

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11. Given the following reaction: 2 HC₂H₂OH (1) + 3 O₂ (g) → 4 CO₂ (g) + 5 H₂ (g) If we started off with 4.88 mL of HC₂H₂OH (density = 1.049 g/mL) at 66.4 °C and a pressure of 3600 mmHg, what volume (L) of hydrogen gas would be produced? 12. The following reaction occurs in the process of fermentation, where glucose (sugar) is broken down into ethanol (the alcohol in cocktails), and carbon dioxide gas. C6H12O6 (aq) → 2 C₂H5OH (1) + 2 CO₂ (g) If we begin with 50.5 g of glucose, what volume (L) of carbon dioxide will be produced? (Hint: this problem combines the stoichiometry of chapter 6, with our new ideal gas law) Assume the reaction takes place at standard temperature and pressure. 11. Given the following reaction: 2 HC₂H₂OH (1) + 3 O₂ (g) → 4 CO₂ (g) + 5 H₂ (g) If we started off with 4.88 mL of HC₂H₂OH (density = 1.049 g/mL) at 66.4 °C and a pressure of 3600 mmHg, what volume (L) of hydrogen gas would be produced? 12. The following reaction occurs in the process of fermentation, where glucose (sugar) is broken down into ethanol (the alcohol in cocktails), and carbon dioxide gas. C6H12O6 (aq) → 2 C₂H5OH (1) + 2 CO₂ (g) If we begin with 50.5 g of glucose, what volume (L) of carbon dioxide will be produced? (Hint: this problem combines the stoichiometry of chapter 6, with our new ideal gas law) Assume the reaction takes place at standard temperature and pressure.

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Q11 Giveng Sol Balanced chemical equation 2HC HOH30g Also given starting wennze DE CONS mart of HCH3... View the full answer