Question

how much heat is produced in burning 2 mol of ch4 inder stnadard conditions if reactants and prodcuts ar brought to 298 K and H2O(l) is formed?

Answer 1

The combustion of 2 mol of CH4 under standard conditions produces 1780.8 kJ of heat when the products are brought to 298 K and H2O is in the liquid state.

Step-by-step explanation:

To answer the question of how much heat is produced in the burning of 2 mol of CH4 under standard conditions while forming H2O(l), we refer to the balanced thermochemical equation for the combustion of methane: CH4(g) + 2O2(g) → CO2(g) + 2H2O(l) + 890.4 kJ. This equation indicates that the combustion of 1 mol of CH4 produces 890.4 kJ of heat.

Using stoichiometry, we can determine the amount of heat produced by 2 mol of CH4. Since the reaction of 1 mol of methane releases 890.4 kJ, the reaction of 2 mol would release:

2 × 890.4 kJ = 1780.8 kJ

Therefore, the burning of 2 mol of CH4 under standard conditions produces 1780.8 kJ when products are brought to 298 K, and H2O is in the liquid state.