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satela [25.4K]
2 years ago
6

My sporty mini van needs 19,126 kJ of energy in order to pass a fast moving street sweeper on the road. Using the following equa

tion, determine how many grams of gasoline (C8H18) will be used up in order to make this happen. 2 C8H18 + 25 O2 --> 16 CO2 + 18 H2O \DeltaΔH = -10,990 kJ
Chemistry
1 answer:
nika2105 [10]2 years ago
8 0

Answer:

m=397.6gC_8H_{18}}

Explanation:

Hello there!

In this case, according to the given chemical reaction, we can set up the heat of reaction per mole of gasoline as shown below:

\Delta H=\frac{-10,990kJ}{2molC_8H_{18}}=-5495\frac{kJ}{molC_8H_{18}}

Now, since the total heat is obtained by multiplying the moles and heat of reaction, we can calculate the moles as shown below:

n=\frac{Q}{-\Delta H } \\\\n=\frac{19,126kJ}{-(-5495\frac{kJ}{molC_8H_{18}} )} \\\\n=3.48molC_8H_{18}}

Finally, since the molar mass of gasoline is 114.22 g/mol, we can easily calculate the mass as follows:

m=3.48molC_8H_{18}} *\frac{114.22gC_8H_{18} }{1molmolC_8H_{18}} } \\\\m=397.6gC_8H_{18}}

Best regards!

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