Question

Gaseous butane will react with gaseous oxygen to produce gaseous carbon dioxide and gaseous water . Suppose 42. g of butane is mixed with 150. g of oxygen. Calculate the maximum mass of carbon dioxide that could be produced by the chemical reaction. Round your answer to significant digits.

Answer 1

The maximum mass of carbon dioxide that could be produced by the chemical reaction between butane and oxygen is 126.1 g.

Step-by-step explanation:

To calculate the maximum mass of carbon dioxide produced by the reaction between butane and oxygen, we need to determine the limiting reagent. The balanced chemical equation for the reaction is:

2 C4H10 + 13 O2 → 8 CO2 + 10 H2O

First, we need to convert the given masses of butane and oxygen to moles using their molar masses (butane: 58.12 g/mol, oxygen: 32.00 g/mol). We divide the mass by the molar mass to get the number of moles. Then, we compare the mole ratios of butane and oxygen in the balanced equation to find the limiting reagent.

After identifying the limiting reagent, we can use the mole ratio between butane and carbon dioxide to calculate the maximum mass of carbon dioxide produced.

Let's calculate it:

1. Convert the mass of butane to moles: 42.0 g butane × (1 mol/58.12 g) = 0.723 mol butane
2. Convert the mass of oxygen to moles: 150.0 g oxygen × (1 mol/32.00 g) = 4.688 mol oxygen
3. Calculate the mole ratio between butane and oxygen: 0.723 mol butane / 2 = 0.362 mol oxygen (approximately)
4. Compare the mole ratio with the actual number of moles of oxygen:

Since the actual number of moles of oxygen (4.688 mol) is greater than the mole ratio comparison (0.362 mol), oxygen is the limiting reagent.

Now, we can use the mole ratio between butane and carbon dioxide to calculate the maximum mass of carbon dioxide:

0.723 mol butane × (8 mol CO2/2 mol butane) × (44.01 g CO2/1 mol CO2) = 126.1 g CO2

Therefore, the maximum mass of carbon dioxide that could be produced by the chemical reaction is 126.1 g.