How much heat is absorbed/released when 35.00 g of NH₃(g) reacts in the presence of excess O₂(g) to produce NO(g) and H₂O(l) according to the following chemical equation?
4 NH₃(g) + 5 O₂(g) → 4 NO(g) + 6 H₂O(l) ΔH° = 1168 kJ

Question

Quizplus · Accepted Answer

We can use the given equation and the given value of ΔH° to calculate the amount of heat absorbed or released in the reaction. First, we need to convert the given mass of NH₃(g) to moles: 35.00 g NH₃(g) x (1 mol NH₃(g) / 168.15 g NH₃(g)) = 0.2082 mol NH₃(g) According to the balanced equation, 4 moles of NH₃(g) produce 1168 kJ of heat. Therefore, 0.2082 moles of NH₃(g) will produce: 1168 kJ x (0.2082 mol / 4 mol) = 60.01 kJ of heat The reaction produces NO(g) and H₂O(l) from NH₃(g) and O₂(g), so it is an endothermic reaction that absorbs heat. Therefore, the correct choice is A) 600.1 kJ of heat are absorbed.

How Much Heat Is Absorbed/released When 35