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The empirical formula of a non-electrolyte is CH2O. A solution containing 6 g of compound exerts the same osmotic pressure as that of 0.05 M glucose solution at same temp. The molecular formula of compound has …….number of atoms in it:
Correct answer is '16'. Can you explain this answer?
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The empirical formula of a non-electrolyte is CH2O. A solution contain...
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The empirical formula of a non-electrolyte is CH2O. A solution contain...
A molecular weight of 90 g/mol.
First, we need to find the molar mass of the compound represented by the empirical formula CH2O:
Molar mass = (12.01 x 1) + (1.01 x 2) + 16.00 = 30.03 g/mol
Next, we can calculate the number of moles of the compound in the solution containing 6 g:
moles = mass / molar mass = 6 g / 30.03 g/mol = 0.1999 mol
Since the osmotic pressure is the same as that of a 0.05 M glucose solution, we can use the van't Hoff factor (i) to calculate the effective concentration of the compound:
i = (osmotic pressure of the solution containing the compound) / (osmotic pressure of a 0.05 M glucose solution)
Assuming both solutions are at the same temperature and volume, the osmotic pressure is directly proportional to the concentration. Therefore:
i = (concentration of the compound) / 0.05 M
Since the compound is a non-electrolyte, i = 1. Therefore:
0.1999 mol / 0.05 M = 3.998 M
Finally, we can use the molar mass and the effective concentration to calculate the molecular formula of the compound:
molecular weight = molar mass x n
n = molecular weight / molar mass = 90 g/mol / 30.03 g/mol = 2.997
The molecular formula is therefore (CH2O)3 or C3H6O3.
First, we need to find the molar mass of the compound represented by the empirical formula CH2O:
Molar mass = (12.01 x 1) + (1.01 x 2) + 16.00 = 30.03 g/mol
Next, we can calculate the number of moles of the compound in the solution containing 6 g:
moles = mass / molar mass = 6 g / 30.03 g/mol = 0.1999 mol
Since the osmotic pressure is the same as that of a 0.05 M glucose solution, we can use the van't Hoff factor (i) to calculate the effective concentration of the compound:
i = (osmotic pressure of the solution containing the compound) / (osmotic pressure of a 0.05 M glucose solution)
Assuming both solutions are at the same temperature and volume, the osmotic pressure is directly proportional to the concentration. Therefore:
i = (concentration of the compound) / 0.05 M
Since the compound is a non-electrolyte, i = 1. Therefore:
0.1999 mol / 0.05 M = 3.998 M
Finally, we can use the molar mass and the effective concentration to calculate the molecular formula of the compound:
molecular weight = molar mass x n
n = molecular weight / molar mass = 90 g/mol / 30.03 g/mol = 2.997
The molecular formula is therefore (CH2O)3 or C3H6O3.
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The empirical formula of a non-electrolyte is CH2O. A solution containing 6 g of compound exerts the same osmotic pressure as that of 0.05 M glucose solution at same temp. The molecular formula of compound has …….number of atoms in it:Correct answer is '16'. Can you explain this answer?
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