Refer to the following unbalanced equation: C6H14+O2->CO2+H2O
What mass of oxygen (O2) is required to react completely with 21.4 g of C6H14?
a. 6.51 × 103 g
b. 37.7 g
c. 7.95 g
d. 75.5 g
e. 0.248 g
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To solve this problem, we need to calculate the molar mass of C6H14 and use it to determine the moles of C6H14. Then, we can use the stoichiometry of the reaction to determine the moles of O2 required and convert it to grams.
The molar mass of C6H14 is:
6 carbon atoms (6 x 12.01 g/mol) + 14 hydrogen atoms (14 x 1.01 g/mol) = 86.18 g/mol
Now we can calculate the moles of C6H14:
21.4 g / 86.18 g/mol = 0.248 mol C6H14
According to the balanced equation, the ratio of C6H14 to O2 is 1:O2. Therefore, the moles of O2 required will be the same as the moles of C6H14.
So, the moles of O2 required = 0.248 mol
Finally, we can convert the moles of O2 to grams:
Grams of O2 = moles of O2 x molar mass of O2
Grams of O2 = 0.248 mol x (2 x 16.00 g/mol) = 7.95 g
Therefore, the mass of O2 required to react completely with 21.4 g of C6H14 is 7.95 g.
The correct answer is: c. 7.95 g.
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