The synthesis of ammonia from nitrogen and oxygen gas is non-spontaneous at 600K, but spontaneous at...

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The synthesis of ammonia from nitrogen and oxygen gas is non-spontaneous at 600K, but spontaneous at standard T of 298K: N2(g) + H2(g) → NH3(g) Is this reaction endothermic or exothermic? endothermic at 298K and exothermic at 600K exothermic at 298K and endothermic at 600K Without values it is impossible to answer this question endothermic at all T exothermic at all T The synthesis of ammonia from nitrogen and oxygen gas is non-spontaneous at 600K, but spontaneous at standard T of 298K: N2(g) + H2(g) → NH3(g) Is this reaction endothermic or exothermic? endothermic at 298K and exothermic at 600K exothermic at 298K and endothermic at 600K Without values it is impossible to answer this question endothermic at all T exothermic at all T The synthesis of ammonia from nitrogen and oxygen gas is non-spontaneous at 600K, but spontaneous at standard T of 298K: N2(g) + H2(g) → NH3(g) Is this reaction endothermic or exothermic? endothermic at 298K and exothermic at 600K exothermic at 298K and endothermic at 600K Without values it is impossible to answer this question endothermic at all T exothermic at all T The synthesis of ammonia from nitrogen and oxygen gas is non-spontaneous at 600K, but spontaneous at standard T of 298K: N2(g) + H2(g) → NH3(g) Is this reaction endothermic or exothermic? endothermic at 298K and exothermic at 600K exothermic at 298K and endothermic at 600K Without values it is impossible to answer this question endothermic at all T exothermic at all T

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1Ans Balance chemical reaction is N2 g 3H2 g 2NH3 g From GibbsHelmholtz equation ... View the full answer