We shall assume that fossil fuel combustion involves the combustion of octane:

2C_{8}H1_{8(l)} + 25O_{2(g)} → 16CO_{2(g)} + 18H_{2}O_{(g)}

Step 1. Determine the mass of CO_{2} produced.

$\mathbf{3}\mathbf{.}\mathbf{7}\mathbf{\times}{\mathbf{10}}^{\mathbf{12}}\overline{)\mathbf{kg}\mathbf{}{\mathbf{C}}_{\mathbf{8}}{\mathbf{H}}_{\mathbf{18}}}\left(\frac{{10}^{3}\overline{)g}}{1\overline{)\mathrm{kg}}}\right)\left(\frac{1\overline{)\mathrm{mol}{C}_{8}{H}_{18}}}{114.23\overline{)g{C}_{8}{H}_{18}}}\right)\left(\frac{16\overline{)\mathrm{mol}{\mathrm{CO}}_{2}}}{2\overline{)\mathrm{mol}{C}_{8}{H}_{18}}}\right)\left(\frac{44.01g{\mathrm{CO}}_{2}}{1\overline{)\mathrm{mol}{\mathrm{CO}}_{2}}}\right)\mathbf{=}$**1.14×10 ^{16} g CO**

Step 2. Determine the volume of the atmosphere.

The world burns approximately 3.7 x 10^{12} kg of fossil fuel per year.

By what percentage does the concentration increase each year due to fossil fuel combustion? Approximate the average properties of the entire atmosphere by assuming that the atmosphere extends from sea level to 15 km and that it has an average pressure of 381 torr and average temperature of 275 K. Assume Earth is a perfect sphere with a radius of 6371 km.

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