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Liquid hexane (CH3(CH2)4CH3) reacts with gaseous oxygen gas (O2) to produce gaseous carbon dioxide (CO2) and gaseous water (H2O). What is the theoretical yield of water formed from the reaction of 62.9 g of hexane and 158. g of oxygen gas?

Be sure your answer has the correct number of significant digits in it.

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Answer:

64.8g of water.

Explanation:

First we must give the balanced reaction equation.

C6H14 + 19/2 O2 ===> 6CO2 + 7H2O ...

moles of hexane present = 62.9g x 1 mole/86 g = 0.73 moles

moles O2 present = 158 g x 1 mole/32g = 4.9 moles

Hence ; oxygen is limiting...

moles of H2O that can be produced

If 9.5 moles of oxygen yields 7 moles of water

4.9 moles of oxygen yields 7×4.9/9.5 = 3.6 moles

Mass of water= 3.6×18= 64.8g of water.

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