Step 1: Understanding the Process.
The given reaction represents the fermentation of glucose, where glucose (\(C_6H_{12}O_6\)) is converted into ethanol (\(C_2H_5OH\)) and carbon dioxide (\(CO_2\)).
Step 2: Identify the Biochemical Pathway.
This is a common biochemical process known as fermentation. In this process, glucose is metabolized by yeast or other microorganisms to produce ethanol and carbon dioxide.
Step 3: Enzyme Catalysis.
The enzyme responsible for this transformation is zymase. Zymase is a complex of enzymes found in yeast that catalyzes the fermentation process. Zymase helps break down glucose into ethanol and carbon dioxide.
Step 4: Verify the Options.
Option (A) Diastase is involved in the breakdown of starch into maltose but not in fermentation.
Option (B) Maltase breaks down maltose into glucose but does not catalyze the fermentation process.
Option (C) Urease is involved in the breakdown of urea, not fermentation.
Option (D) Xylose is incorrect because it is a sugar, not an enzyme.
Therefore, the correct enzyme for this transformation is zymase, which is involved in the fermentation of glucose.
Match the LIST I (Enzyme) with LIST II (Catabolic Products)
| LIST-I | LIST-II | ||
|---|---|---|---|
| (Enzyme) | (Catabolic Products) | ||
| A | \(\beta\)-galactosidase | III | Galactose + glucose |
| B | Lecithinase | I | Choline + H$_3$PO$_4$ + fat |
| C | Urease | IV | CO$_2$ + NH$_3$ |
| D | Lipase | II | Glycerol + fatty acids |
At 15 atm pressure, $ \text{NH}_3(g) $ is being heated in a closed container from 27°C to 347°C and as a result, it partially dissociates following the equation: $ 2\text{NH}_3(g) \rightleftharpoons \text{N}_2(g) + 3\text{H}_2(g) $ If the volume of the container remains constant and pressure increases to 50 atm, then calculate the percentage dissociation of $ \text{NH}_3(g) $
If equilibrium constant for the equation $ A_2 + B_2 \rightleftharpoons 2AB \quad \text{is} \, K_p, $ then find the equilibrium constant for the equation $ AB \rightleftharpoons \frac{1}{2} A_2 + \frac{1}{2} B_2. $
Consider the following reaction: $ \text{CO}(g) + \frac{1}{2} \text{O}_2(g) \rightarrow \text{CO}_2(g) $ At 27°C, the standard entropy change of the process becomes -0.094 kJ/mol·K. Moreover, standard free energies for the formation of $ \text{CO}_2(g) $ and $ \text{CO}(g) $ are -394.4 and -137.2 kJ/mol, respectively. Predict the nature of the above chemical reaction.