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What volume of hydrogen could be produced from 256 g of glucose at STP?

What volume of hydrogen could be produced from 256 g of glucose at STP?

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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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**Question:** What volume of hydrogen could be produced from 256 g of glucose at STP? --- **Explanation:** This question is about determining the amount of hydrogen gas that can be produced from a specific mass of glucose (256 grams) under Standard Temperature and Pressure (STP) conditions. You would typically use stoichiometry, taking into account the balanced chemical equation for the reaction, molar masses, and the fact that at STP, one mole of an ideal gas occupies 22.4 liters. To solve this, you need to consider: 1. The chemical equation for the decomposition or reaction of glucose. 2. The molar mass of glucose and hydrogen. 3. The conversion of mass of glucose to moles, and then to moles of hydrogen. 4. The conversion from moles of hydrogen to volume at STP (using 22.4 L/mol as the molar volume for gases at STP).
Transcribed Image Text:**Question:** What volume of hydrogen could be produced from 256 g of glucose at STP? --- **Explanation:** This question is about determining the amount of hydrogen gas that can be produced from a specific mass of glucose (256 grams) under Standard Temperature and Pressure (STP) conditions. You would typically use stoichiometry, taking into account the balanced chemical equation for the reaction, molar masses, and the fact that at STP, one mole of an ideal gas occupies 22.4 liters. To solve this, you need to consider: 1. The chemical equation for the decomposition or reaction of glucose. 2. The molar mass of glucose and hydrogen. 3. The conversion of mass of glucose to moles, and then to moles of hydrogen. 4. The conversion from moles of hydrogen to volume at STP (using 22.4 L/mol as the molar volume for gases at STP).
Generating hydrogen from water or methane is energy-intensive. A non-natural enzymatic process has been developed that produces 12 moles of hydrogen per mole of glucose by the reaction: \[ \text{C}_6\text{H}_{12}\text{O}_6\; (aq) + 6\text{H}_2\text{O}\; (l) \longrightarrow 12\text{H}_2\; (g) + 6\text{CO}_2\; (g) \] In this reaction, aqueous glucose (C₆H₁₂O₆) reacts with liquid water (H₂O) to produce gaseous hydrogen (H₂) and gaseous carbon dioxide (CO₂). This process exemplifies an innovative approach to hydrogen production, using glucose as a feedstock.
Transcribed Image Text:Generating hydrogen from water or methane is energy-intensive. A non-natural enzymatic process has been developed that produces 12 moles of hydrogen per mole of glucose by the reaction: \[ \text{C}_6\text{H}_{12}\text{O}_6\; (aq) + 6\text{H}_2\text{O}\; (l) \longrightarrow 12\text{H}_2\; (g) + 6\text{CO}_2\; (g) \] In this reaction, aqueous glucose (C₆H₁₂O₆) reacts with liquid water (H₂O) to produce gaseous hydrogen (H₂) and gaseous carbon dioxide (CO₂). This process exemplifies an innovative approach to hydrogen production, using glucose as a feedstock.
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