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3 years ago

PLEASE SOMEONE HELP ME WITH THIS

Chemistry

1 answer:

Likurg_2 [28]3 years ago

3 0

Answer:

1.30 moles

Explanation:

As written, the molar mass of the fat is 770.5 g/mole. Add all the C, H, and O's (I get C48H98O6) and multiply by the molar mass of each. I obtain the 770.5 grams/mole figure, but would note that a more common fat is actually C3H5(O<u>H</u>(CH2)14(CH3))3 and not C3H5(O<u>O</u>(CH2)14(CH3))3.

Assuming C3H5(OO(CH2)14(CH3))3 is the correct structure, 1000g would mean 1000g/(770.5 g/mole) = 1.298 moles, or 1.30 moles to 2 sig figs.

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A. The balanced equation for the reaction is

2C₂H₂ + 5O₂ —> 4CO₂ + 2H₂O

B. The volume of the oxygen gas required to burn 0.700 L of acetylene gas is 1.75 L

C. The volume of carbon dioxide gas produced is 1.4 L

D. The volume of water vapor produced is 0.7 L

<h3>A. Balanced equation </h3>

The balanced equation for the reaction between acetylene gas (C₂H₂) and oxygen gas (O₂) is given below

2C₂H₂ + 5O₂ —> 4CO₂ + 2H₂O

<h3>B. How to determine the volume of oxygen </h3>

2C₂H₂ + 5O₂ —> 4CO₂ + 2H₂O

Since the reaction occurred at standard temperature and pressure, we can thus say that:

From the balanced equation above,

2 L of C₂H₂ reacted with 5 L O₂.

Therefore,

0.7 L of C₂H₂ will react with = (0.7 × 5) / 2 = 1.75 L of O₂

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<h3>C. How to determine the volume of carbon dioxide </h3>

2C₂H₂ + 5O₂ —> 4CO₂ + 2H₂O

From the balanced equation above,

2 L of C₂H₂ reacted to produce 4 L of CO₂

Therefore,

0.7 L of C₂H₂ will react to produce = (0.7 × 4) / 2 = 1.4 L of CO₂

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<h3>D. How to determine the volume of water. </h3>

2C₂H₂ + 5O₂ —> 4CO₂ + 2H₂O

From the balanced equation above,

2 L of C₂H₂ reacted to produce 2 L of H₂O

Therefore,

0.7 L of C₂H₂ will also react to produce 0.7 L of H₂O

Thus, 0.7 L of H₂O was produced

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