Calculate the theoretical yield of carbon dioxide from the combustion of 10.4 g of butanol in the presence of 25.1 g of oxygen gas.C4H10O  +  6 O2  -->  4 CO2  +  5 H2O

First, we need to calculate the molar mass of butanol (C4H10O) and oxygen (O2).

The molar mass of butanol is calculated as follows: C: 12.01 g/mol x 4 = 48.04 g/mol H: 1.01 g/mol x 10 = 10.1 g/mol O: 16.00 g/mol x 1 = 16.00 g/mol Total molar mass of butanol = 48.04 g/mol + 10.1 g/mol + 16.00 g/mol = 74.14 g/mol

The molar mass of oxygen (O2) is: O: 16.00 g/mol x 2 = 32.00 g/mol

Next, we calculate the number of moles of butanol and oxygen: Moles of butanol = 10.4 g / 74.14 g/mol = 0.14 mol Moles of oxygen = 25.1 g / 32.00 g/mol = 0.78 mol

From the balanced chemical equation, we know that 1 mol of butanol reacts with 6 mol of oxygen to produce 4 mol of carbon dioxide.

Therefore, the theoretical yield of carbon dioxide from the combustion of butanol can be calculated as follows:

From butanol: 0.14 mol butanol x (4 mol CO2 / 1 mol butanol) = 0.56 mol CO2 From oxygen: 0.78 mol O2 x (4 mol CO2 / 6 mol O2) = 0.52 mol CO2

The limiting reagent is the one that produces the least amount of product, which in this case is oxygen. Therefore, the theoretical yield of CO2 is 0.52 mol.

To convert this to grams, we multiply by the molar mass of CO2: 0.52 mol CO2 x 44.01 g/mol CO2 = 22.9 g CO2

So, the theoretical yield of carbon dioxide from the combustion of 10.4 g of butanol in the presence of 25.1 g of oxygen gas is 22.9 g.