. Determine the mass of carbon dioxide produced when 0.85 grams of butane (C4 H10 ) reacts with oxygen according to the following balanced chemical equation: 2 C4 H10 + 13 O2 → 8 CO2 + 10 H2 O

Step 1: Calculate the molar mass of butane (C4H10) The molar mass of butane is calculated by adding the molar masses of its constituent atoms. The molar mass of carbon (C) is approximately 12.01 g/mol, and there are 4 carbon atoms in butane. The molar mass of hydrogen (H) is approximately 1.01 g/mol, and there are 10 hydrogen atoms in butane.

So, the molar mass of butane = (4 * 12.01 g/mol) + (10 * 1.01 g/mol) = 58.14 g/mol

Step 2: Calculate the number of moles of butane The number of moles of a substance is calculated by dividing the mass of the substance by its molar mass. So, the number of moles of butane = 0.85 g / 58.14 g/mol = 0.0146 mol

Step 3: Use the stoichiometry of the reaction to find the number of moles of carbon dioxide From the balanced chemical equation, we can see that 2 moles of butane produce 8 moles of carbon dioxide. So, 0.0146 moles of butane will produce = 0.0146 mol * (8 mol CO2 / 2 mol C4H10) = 0.0584 mol of CO2

Step 4: Calculate the mass of carbon dioxide The molar mass of carbon dioxide (CO2) is calculated by adding the molar masses of its constituent atoms. The molar mass of carbon (C) is approximately 12.01 g/mol, and there is 1 carbon atom in CO2. The molar mass of oxygen (O) is approximately 16.00 g/mol, and there are 2 oxygen atoms in CO2.

So, the molar mass of CO2 = (1 * 12.01 g/mol) + (2 * 16.00 g/mol) = 44.01 g/mol

Finally, the mass of CO2 produced = 0.0584 mol * 44.01 g/mol = 2.57 g

So, 0.85 g of butane will produce approximately 2.57 g of carbon dioxide when it reacts with oxygen.