Calculate the amount of energy released when 3.60 kg of butane (C4H10) is burnt in an unlimited supply of oxygen.?

We gots a combustion reaction....

To calculate the amount of energy released when 3.60 kg of butane (C4H10) is burnt in an unlimited supply of oxygen, we first need to determine the molar mass of butane.

The molar mass of butane (C4H10) can be calculated as follows:

Molar mass of carbon (C) = 12.01 g/mol Molar mass of hydrogen (H) = 1.01 g/mol

Molar mass of butane (C4H10) = (4 × molar mass of carbon) + (10 × molar mass of hydrogen) = (4 × 12.01 g/mol) + (10 × 1.01 g/mol) = 48.04 g/mol + 10.10 g/mol = 58.14 g/mol

Next, we calculate the number of moles of butane in 3.60 kg:

Number of moles = Mass / Molar mass = 3600 g / 58.14 g/mol ≈ 61.90 mol

The balanced chemical equation for the combustion of butane is:

2 C4H10 + 13 O2 → 8 CO2 + 10 H2O

From the balanced equation, we see that 2 moles of butane produce 8 moles of CO2 and 10 moles of H2O. Therefore, 61.90 moles of butane will produce:

8 × 61.90 ≈ 495.20 moles of CO2 10 × 61.90 ≈ 619.00 moles of H2O

Next, we need to calculate the energy released per mole of butane burnt. The standard enthalpy of combustion of butane is -2878 kJ/mol.

The total energy released when 61.90 moles of butane are burnt is:

Energy released = Number of moles × Enthalpy change = 61.90 mol × -2878 kJ/mol ≈ -177969.20 kJ

Therefore, when 3.60 kg of butane is burnt in an unlimited supply of oxygen, approximately 177969.20 kJ of energy is released.