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How many grams of water will be produced when 1.6 moles of ethanol (CH3CH2OH) are burned completely? Enter a number only (no units) and express your answer using the correct number of significant figures.

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maacastrobr

Answer:

86

Explanation:

The reaction that takes place is:

  • C₂H₅OH + 3O₂ → 2CO₂ + 3H₂O

First we convert moles of ethanol to moles of water:

  • 1.6 mol ethanol * [tex]\frac{3molH_2O}{1molEthanol}[/tex] = 4.8 mol H₂O

Then we convert moles of water to grams of water, using its molar mass:

  • 4.8 mol H₂O * 18 g/mol = 86.4 g

So 84.6 grams of water will be produced.

Eduard22sly

The mass of water, H₂O produced when 1.6 moles of ethanol, C₂H₅OH are completely burned is 86.4 g

We'll begin by writing the balanced equation for the reaction. This is given below

C₂H₅OH + 3O₂ → 2CO₂ + 3H₂O

From the balanced equation above,

1 mole of C₂H₅OH reacted to produce 3 moles of H₂O.

  • Next, we shall determine the number of mole of H₂O produced by the reaction of 1.6 moles of C₂H₅OH

From the balanced equation above,

1 mole of C₂H₅OH reacted to produce 3 moles of H₂O.

Therefore,

1.6 moles of C₂H₅OH will react to produce = 1.6 × 3 = 4.8 moles of H₂O.

  • Finally, we shall determine the mass of 4.8 moles of H₂O.

Mole of H₂O = 4.8 moles

Molar mass of H₂O = (2×1) + 16 = 18 g/mol

Mass of H₂O =?

Mass = mole × molar mass

Mass of H₂O = 4.8 × 18

Mass of H₂O = 86.4 g

Thus, the mass of water obtained from the reaction is 86.4 g

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