Help with Enthalpy Practice Test

Consider these two half reactions:

Step 1. $CH_{4}{(g)} + 2O{2}{(g)} \rightarrow CO{2}{(g)} + 2H{2}O_{(l)}$ $\Delta H = -890kJ$

Step 2. $H_{2}O_{(l)} \rightarrow H_{2}O_{(g)}$ $\Delta H = 44kJ$

Based on these half reactions, find the enthalpy for the following reaction:

$CH_{4}{(g)} + 2O{2}{(g)} \rightarrow CO{2}{(g)} + 2H{2}O_{(g)}$

Consider the following balanced reaction:

$2C_{(s)} + 3H_{2}{(g)} \rightarrow C{2}H_{6}_{(g)}$

$\Delta H = -84kJ$

What is the change in enthalpy if $\small 10g$ of solid carbon is used in the above reaction?