Consider the following unbalanced equation: If 1.70 g of ethanol reacts with 11.2 g of oxygen, how many moles of carbon dioxide are produced?

Question

Consider the following unbalanced equation:  If 1.70 g of ethanol reacts with 11.2 g of oxygen, how many moles of carbon dioxide are produced?

Quizplus · Accepted Answer

First, we need to balance the equation:

C2H5OH + 3O2 -> 2CO2 + 3H2O

Next, we convert the given masses to moles:

1.70 g C2H5OH / 46.07 g/mol C2H5OH = 0.0369 mol C2H5OH

11.2 g O2 / 32.00 g/mol O2 = 0.350 mol O2

Now, we need to determine the limiting reactant. To do this, we calculate the mole ratio of each reactant to the product:

Mole ratio for C2H5OH:

1 mol C2H5OH / 2 mol CO2

Mole ratio for O2:

3 mol O2 / 2 mol CO2

Since the mole ratio for C2H5OH is lower, it is the limiting reactant. We can use the mole ratio from the balanced equation to determine the amount of CO2 produced:

1 mol C2H5OH produces 2 mol CO2

0.0369 mol C2H5OH x (2 mol CO2 / 1 mol C2H5OH) = 0.0738 mol CO2

Therefore, the answer is C) 0.0738 mol CO2.

Consider the Following Unbalanced Equation: If 1