Question

For the combustion of 1 mole of cyclohexane at 25 c and 1.0 bar calculate the work that must be done

Answer 1

To calculate the work that must be done for the combustion of 1 mole of cyclohexane at 25°C and 1.0 bar, we need to consider the change in volume and pressure.

The work done can be calculated using the equation:

Work = -PΔV

Where P is the pressure and ΔV is the change in volume.

Since we have the pressure (1.0 bar), we need to determine the change in volume.

Answer 2

The work done against the atmosphere for the expansion of gaseous products from the combustion of 1.00 mol of cyclohexane is -9.917 kJ. This is calculated using the ideal gas law and the formula for work at constant pressure.

Step-by-step explanation:

The combustion of 1.00 mol of cyclohexane, C6H12, produces gaseous products which expand and do work against the atmosphere. To calculate this work, we can use the formula for work done by a gas at constant pressure:

W = -PΔV

where W is work, P is the external pressure and ΔV is the change in volume. Since we're at 1.00 bar (100 kPa), we need the change in volume in cubic meters. For the combustion reaction:

2 C6H12(l) + 19 O2(g) → 12 CO2(g) + 12 H2O(g)

Using stoichiometry, we find that 1 mol of cyclohexane produces a total of 12 moles of gaseous products. Now, using the ideal gas law at 25 °C:

ΔV = nRT/P = (12 mol)(0.08314 L9)/(100 kPa) = 0.09917 m^3

Finally, we calculate the work done:

W = -(100 kPa)(0.09917 m^3)

W = -9.917 kJ (since 1 kPam^3 = 1 J)

Therefore, the work done against the atmosphere for the expansion of the gaseous products is -9.917 kJ.