Final answer:
The reaction of 2.0 mol CH₄ (g) with 2.0 mol O₂ (g) is exothermic and would release 426 kcal of heat, as each mole of CH₄ releases 213 kcal upon reaction.
Step-by-step explanation:
The student's question about how much heat is absorbed or released when 2.0 mol of CH₄ (g) reacts with 2.0 mol of O₂ (g) relates to the exothermic or endothermic nature of the reaction. The provided information shows that when 1 mol of CH₄ (g) reacts with 2 O₂ (g), it produces CO₂ (g) and 2H₂O (l) and releases 213 kcal (or 890.4 kJ) of heat. This indicates that the reaction is exothermic, as it releases heat into the surroundings.
For 2.0 mol of CH₄ (g), the amount of heat released would be 2 times the amount released for 1 mole. To calculate this, simply multiply 213 kcal by 2, which equates to 426 kcal released. Thus, when 2.0 mol of CH₄ reacts with 2.0 mol of O₂, the reaction is exothermic and would release a total of 426 kcal of heat.