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Answer :
Final answer:
To make a 1.55 m solution of glucose in 350.0 g of water, 97.7 grams of glucose are required. Thus, option 4) 97.7 is correct answer.
Explanation:
The question asks how many grams of glucose are needed to make a 1.55 m (molal) solution, when dissolved in 350.0 g of water. Molality (m) is defined as the number of moles of solute per kilogram of solvent. To find the mass of glucose needed, we first calculate the moles of glucose required and then translate this to grams using glucose's molar mass. Given that the molality is 1.55 m, this means we need 1.55 moles of glucose per kilogram of water. Since we have 0.350 kg of water (350.0 g), the moles of glucose required are 1.55 mol/kg * 0.350 kg = 0.5425 mol. The molar mass of glucose (C6H12O6) is approximately 180.2 g/mol, so the mass of glucose needed is 0.5425 mol * 180.2 g/mol = 97.7 grams.
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