The value of ΔH° for the reaction below is -336 kJ. Calculate the heat (kJ)released to the surroundings when 23.0 g of HCl is formed. CH₄ (g)+ 3 Cl₂ (g)→ CHCl₃ (l)+ 3HCl (g)

Question

Quizplus · Accepted Answer

First, we need to calculate the moles of HCl produced:
23.0 g HCl x 1 mol HCl/ 36.46 g HCl = 0.631 mol HCl

Next, we can use the given ΔH° value and the stoichiometry of the reaction to calculate the heat released:
-336 kJ/ 3 mol HCl x 0.631 mol HCl = -70.7 kJ

Since the reaction releases heat to the surroundings, the value is negative, and the absolute value of -70.7 kJ is 70.7 kJ. Therefore, the correct answer is C) 70.7.

The Value of ΔH° for the Reaction Below Is -336