Question 1
When 1.50 mol of CH4(g) reacts with excess Cl2(g) at constant pressure according to the chemical equation shown below, 1062 kJ of heat are released. Calculate the value of ΔH for this reaction, as written.2CH4(g) + 3Cl2(g) → 2CHCl3(l) + 3H2(g) | Δ rH° = ? |
Question 2
In the presence of excess oxygen, methane gas burns in a constant pressure system to yield carbon dioxide and water:CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O (l) | Δ rH = -890.0 kJ |
Answer 1
-1420 kJ mol-1Answer 2
-106 kJ mol-1