Consider the reaction, C₂H₄(g)+ H₂(g)$\rightarrow$C₂H₆(g), where $\Delta$H = -137 kJ. How many kilojoules are released when 3.5 mol of C₂H₄reacts?

Question

Quizplus · Accepted Answer

According to the balanced equation, 2 mol of C₂H₄ reacts to release 137 kJ of energy. Therefore, 1 mol of C₂H₄ will release 137/2 = 68.5 kJ of energy. To calculate the energy released when 3.5 mol of C₂H₄reacts, we can use the concept of proportionality. - 2 mol of C₂H₄ releases 137 kJ of energy - 1 mol of C₂H₄ releases 68.5 kJ of energy - Therefore, 3.5 mol of C₂H₄ will release (3.5 mol / 1 mol) x (68.5 kJ/mol) = 239.8 kJ of energy Therefore, the correct answer is C) 480 kJ are released.

Consider the Reaction, C2H4(g)+ H2(g) →\rightarrow→ C2H6(g), Where Δ\DeltaΔ H = -137 KJ

Consider the Reaction, C₂H₄(g)+ H₂(g) $\rightarrow$ C₂H₆(g), Where $\Delta$ H = -137 KJ