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Answer :
Final answer:
To find the grams of sucrose in a 1.55 L 0.758M solution, we multiply the moles of sucrose (calculated from the solution's molarity and volume) by the molar mass of sucrose. However, the calculation provided does not match the options given, suggesting an error or misunderstanding in the calculation process. So, the correct option is not given.
Explanation:
To find the grams of sucrose in a 1.55 L of a 0.758M sucrose solution, we first need to calculate the number of moles of sucrose present in the solution. Molarity (M) is defined as the number of moles of solute per liter of solution. Therefore, the number of moles of sucrose can be calculated using the formula: molarity (M) = moles of solute / liters of solution, Given that the molarity of the sucrose solution is 0.758M and the volume of the solution is 1.55L, we can rearrange the formula to solve for moles of sucrose: moles of sucrose = molarity (M) × liters of solution = 0.758 mol/L × 1.55 L.
After calculating the moles of sucrose, we multiply by the molar mass of sucrose to find the grams of sucrose present in the solution. The molar mass of sucrose (C12H22O11) is 342.297g/mol. Grams of sucrose = moles of sucrose × molar mass of sucrose. After performing the calculations:
- Moles of sucrose = 1.17569 moles
- Grams of sucrose = 1.17569 moles × 342.297g/mol
The final calculation yields 402.339 grams of sucrose, which does not match any of the provided options, indicating a possible error in calculation or misunderstanding of the provided question. For the purpose of aligning with the options given, the closest calculation process and understanding of the question leads to:
Using the correct approach, the exact answer would be found by accurately calculating moles of sucrose and then converting those moles to grams using the molar mass. The discrepancies might come from a misunderstanding of the calculation or the initial information provided. It is crucial to ensure all values and formulas are applied correctly in chemistry calculations.
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