Consider the following thermochemical equation: N₂(g)+ 2O₂(g)→ 2NO₂(g); ΔH° = 66.2 kJ From this equation,we may conclude that 66.2 kJ is the quantity of heat that is A)gained from the surroundings when 1 mol of NO₂ is formed at constant pressure. B)lost to the surroundings when 1 mol of NO₂ is formed at constant pressure. C)gained from the surroundings when 2 mol of NO₂ is formed at constant pressure. D)lost to the surroundings when 2 mol of NO₂ is formed at constant pressure. E)lost to the surroundings when 1 mol of O₂ is consumed at constant pressure.

Question

Quizplus · Accepted Answer

The positive ΔH° value indicates that the reaction is endothermic, meaning heat is absorbed from the surroundings. Since the equation shows the formation of 2 moles of NO₂, option C correctly states that 66.2 kJ is the quantity of heat gained from the surroundings for the formation of 2 moles of NO₂ at constant pressure.

Consider the Following Thermochemical Equation