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zloy xaker [14]
3 years ago
7

How many grams of sucrose (C12H22O11) are in 1.55 L of 0.758 M sucrose solution?

Chemistry
1 answer:
victus00 [196]3 years ago
6 0

Answer:

Mass of Sucrose in given Solution is 401.8158 grams.

Explanation:

Given,

Molarity  of Sucrose Solution = 0.758 M.

Volume of Sucrose Solution(V) = 1.55 L.

To find the mass of Sucrose in the solution, we need to find the number of moles of Sucrose present in the given solution 0f 0.758 M.

c = 0.758 M

number of moles can be calculated using

n = c*V

n= 0.758*1.55  = 1.1749 moles

Then to convert no, of moles to mass, we can use the formula,

number of moles(n) = Mass(m)/Molar Mass(M)

The Molar mass of Sucrose C₁₂H₂₂O₁₁ is

Mass of Carbon Sucrose = 12*12 = 144  grams

Mass of Hydogen in Sucrose = 1*22 = 22 grams

Mass of Oxygen in Sucrose = 16*11 = 176 grams

Molar mass of Sucrose = 144 + 22 +176 = 342 grams.

Substituting the values in the formula,

number of moles(n) = Mass(m)/Molar Mass(M)

we get,

1.1749 = (m)/342 => m = 1.1749 *342 = 401.8158 grams.

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Answer:

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Explanation:

To solve this question we need to find the molecular formula of the compounds converting the mass of each atom to moles. Molecular formula is defined as the simplest whole number ratio of atoms present in a molecula:

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<em>Moles Tin: </em>

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Compounds 1 and 2 are not the same because molecular formulas are different.

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2 years ago
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