How many moles of isooctane must be burned to produce 100 kJ of heat under standard state conditions?

To determine the number of moles of isooctane that must be burned to produce 100 kJ of heat under standard state conditions, we can use the concept of molar enthalpy of combustion.

1. First, we need to find the molar enthalpy of combustion of isooctane. This value represents the amount of heat released when one mole of isooctane is completely burned. Let's assume the molar enthalpy of combustion of isooctane is -5500 kJ/mol.

2. Next, we can use the equation:

   q = n * ΔH

   where q is the heat released (100 kJ), n is the number of moles of isooctane, and ΔH is the molar enthalpy of combustion.

3. Rearranging the equation, we have:

   n = q / ΔH

   Plugging in the values, we get:

   n = 100 kJ / -5500 kJ/mol

4. Calculating the result, we find:

   n ≈ -0.018 mol

   Since moles cannot be negative, we can conclude that approximately 0.018 moles of isooctane must be burned to produce 100 kJ of heat under standard state conditions.