Consider the reaction, 3 NO₂(g)+ H₂O(l)$\rightarrow$ 2 HNO₃(aq)+ NO(g), where $\Delta$H = -137 kJ. How many kilojoules are released when 92.3 g of NO₂reacts?

Question

Quizplus · Accepted Answer

1. Calculate the moles of NO₂: 92.3 g NO₂ × (1 mol NO₂ / 92.12 g NO₂) = 1 mol NO₂ 2. Use stoichiometry to find the moles of NO produced: 1 mol NO₂ × (1 mol NO / 3 mol NO₂) = 0.333 mol NO 3. Calculate the heat released: q = ΔH°rxn × n q = (-137 kJ/mol) × (0.333 mol) q = -45.6 kJ Note: The negative sign indicates that the reaction is exothermic and releases heat.

Consider the Reaction, 3 NO2(g)+ H2O(l) →\rightarrow→ 2 HNO3(aq)+ NO(g), Where Δ\DeltaΔ

Consider the Reaction, 3 NO₂(g)+ H₂O(l) $\rightarrow$ 2 HNO₃(aq)+ NO(g), Where $\Delta$