When 0.236 mol of a weak base (A^-)is reacted with excess HCl,6.91 kJ of energy is released as heat.What is $\Delta$H for this reaction per mole of A^- consumed?

Question

Quizplus · Accepted Answer

The heat released in the reaction is given by the equation: q = nA^-× F1F1F1S1F1F1F10H where nA^- is the amount of weak base consumed. Rearranging the equation gives: F1F1F1S1F1F1F10H = q/nA^- Substituting the given values, we get: F1F1F1S1F1F1F10H = -6.91 kJ/0.236 mol F1F1F1S1F1F1F10H = -29.3 kJ/mol Therefore, the correct answer is C.

When 0236 Mol of a Weak Base (A-)is Reacted with Excess

When 0236 Mol of a Weak Base (A^-)is Reacted with Excess