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| The enthalpy change for the formation of NO(g) from its elements, as indicated below, cannot be measured directly because the reaction is reactant favoured. | Die entalpieverandering vir die vorming van NO(g) vanaf sy elemente, soos hieronder aangedui, kan nie direk bepaal word nie, want die reaksie is reaktant gedrewe. |
Use Hess's Law as well as the enthalpy changes for the reactions below, which was determined experimentally, to determine the enthalpy change (in kJ) of formation for NO(g). | Gebruik Hess se Wet sowel as die entalpieveranderinge vir die reaksies hieronder, wat eksperimenteel bepaal is, om die entalpieverandering (in kJ) vir die vorming van NO(g) te bepaal. |
N2(g) + 3 H2(g) → 2 NH3(g) ΔHo = -91.1 kJ. mol-1 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g) ΔHo = -906.2 kJ.mol-1 H2(g) + |
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