Methane cannot be made cleanly from carbon and hydrogen, so its Δf H° is found with Hess's law…

Step 1. The target. $\text{C(graphite)} + 2\text{H}_2\text{(g)} \rightarrow \text{CH}_4\text{(g)}$.

Step 2. The steps. Burn the carbon: $-393.5\ \text{kJ}$. Burn two moles of hydrogen: $2 \times (-285.8) = -571.6\ \text{kJ}$. Reverse the burning of methane: $+890.3\ \text{kJ}$.

Step 3. Add. The $\text{CO}_2$, the water and the oxygen all cancel. $\Delta_f H^\ominus = -393.5 - 571.6 + 890.3 = -74.8\ \text{kJ mol}^{-1}$.