How much heat is absorbed/released when 10.00 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

The chemical equation shows that the reaction is endothermic, with a positive value for ΔH°. Thus, heat is absorbed during the reaction. To calculate the amount of heat absorbed, we need to use the given mass of NH₃(g) and the molar enthalpy of reaction: - Calculate the moles of NH₃(g): 10.00 g / molar mass of NH₃(g) = 0.0575 mol - Use the molar ratio from the balanced equation to find the moles of O₂(g) consumed: 5 mol O₂(g) / 4 mol NH₃(g) x 0.0575 mol NH₃(g) = 0.0719 mol - Calculate the heat absorbed by the reaction: q = ΔH° x n = +1168 kJ/mol x 0.0575 mol = +67.1 kJ - The positive sign indicates that heat is absorbed by the reaction, so the answer is A: 171.5 kJ of heat are absorbed.

How Much Heat Is Absorbed/released When 10