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Phoenix [80]
3 years ago
10

How many grams of SnO2 are required to produce 1.20x10^21 molecules of water?

Chemistry
1 answer:
Drupady [299]3 years ago
8 0

Answer:

  • <u>0.150 grams</u>

<u></u>

Explanation:

The balanced chemical reaction to obtain water from SnO₂ is:

  • SnO₂ + 2H₂ → Sn + 2H₂O

The mole ratio is:

          \dfrac{1molSnO_2}{2molH_2O}

Find the number of moles equivalent to  1.20× 10²¹ molecules of water, using Avogadro's number:

         1.20\times 10^{21}molecules\times \dfrac{1mol}{6.022\times 10^{23}molecules}=1.9927\times 10^{-3}moles

From the mole ratio, the number of moles of SnO₂ are half the number of moles of water. That is:

  • 0.0019927 moles / 2 = 0.00099635 moles of SnO₂

Use the molar mass of SnO₂ to convert the number of moles to grams:

  • molar mass of SnO₂ = 150.71g/mol
  • mass of SnO₂ = 0.00099635mol × 150.71 g/mol = 0.150 grams.

The answer must be reported with 3 significant figures.

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Answer:

The answer to your question is the mass of solute = 53.5 g

Explanation:

Data

mass of solution = 482 g

mass of solute = ?

mass percent = 11.1 %

Mass percent is a unit of concentration. It measures the mass of the solute divided by the total mass of the solution

Process

1.- Write the formula

        Mass percent = mass of solute / mass of solution x 100

-Solve for mass of solute

          mass of solute = Mass percent x mass of solution / 100

2.- Substitution

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3.- Simplification

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4.- Result

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