From July 2008 changes will apply to the way in which taxes are levied on new cars bought in Ireland - Leaving Cert Chemistry - Question b - 2008

Using the molar mass of CO₂ (44 g/mol), we calculate the number of moles as follows:

$ext{Number of moles} = \frac{\text{Mass of CO₂}}{\text{Molar mass of CO₂}}$

$= \frac{1144 ext{ g}}{44 ext{ g/mol}} = 26 ext{ mol}$

At room temperature and pressure, one mole of gas occupies approximately 24 liters. Therefore, the total volume of CO₂ produced is:

$\text{Volume of CO₂} = \text{Number of moles} \times 24 ext{ L/mol}$

Calculating this gives:

$\text{Volume of CO₂} = 26 ext{ mol} \times 24 ext{ L/mol} = 624 ext{ L}$

For the large SUV with an emission of 264 g CO₂/km, we first calculate the total emission:

$\text{Mass of CO₂ (SUV)} = 264 ext{ g/km} \times 8 ext{ km} = 2112 ext{ g}$

The difference in mass produced by using the SUV:

$\text{Difference in mass} = 2112 ext{ g} - 1144 ext{ g} = 968 ext{ g}$

Next, to find how many liters of this difference would be released:

$\text{Additional volume} = \frac{968 ext{ g}}{44 ext{ g/mol}} \times 24 ext{ L/mol} = 528 ext{ L}$