Consider the following unbalanced equation:
C2H5OH + O2 -> CO2 + H2O
If 1.18 g of ethanol reacts with 14.1 g of oxygen, how many moles of carbon dioxide are produced?
a. 0.0256 mol
b. 0.294 mol
c. 0.0512 mol
d. 0.441 mol
e. 0.0128 mol
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To find the moles of carbon dioxide produced, we need to balance the equation first:
C2H5OH + O2 -> CO2 + H2O
The balanced equation is:
2 C2H5OH + 3 O2 -> 2 CO2 + 3 H2O
Next, we need to find the limiting reactant, which is the reactant that is completely consumed in the reaction. To do this, we can convert the mass of each reactant to moles.
1.18 g of ethanol (C2H5OH):
Molar mass of C2H5OH = 2(12.01 g/mol) + 6(1.008 g/mol) + 1(16.00 g/mol) = 46.07 g/mol
Moles of C2H5OH = 1.18 g / 46.07 g/mol = 0.0256 mol
14.1 g of oxygen (O2):
Molar mass of O2 = 2(16.00 g/mol) = 32.00 g/mol
Moles of O2 = 14.1 g / 32.00 g/mol = 0.441 mol
From the balanced equation, we can see that for every 2 moles of C2H5OH, 2 moles of CO2 are produced. Therefore, the moles of CO2 produced would be:
0.0256 mol C2H5OH * (2 mol CO2 / 2 mol C2H5OH) = 0.0256 mol CO2
Therefore, the number of moles of carbon dioxide produced is 0.0256 mol.
The correct answer is:
a. 0.0256 mol
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