hydrochloric acid reacts with barium hydroxide according to the equation : 2HCl(aq)+Ba(OH)2(AQ)->BaCl2(aq)+2H2O(l) DeltaH= -118 kj Calculate the heat (in kj) associated with the complete reaction of 36.5 grams of HCl (aq)
The Correct Answer and Explanation is :
Explanation:
The balanced chemical equation for the reaction between hydrochloric acid (HCl) and barium hydroxide (Ba(OH)₂) is: 2HCl(aq)+Ba(OH)2(aq)→BaCl2(aq)+2H2O(l)2HCl(aq) + Ba(OH)_2(aq) \rightarrow BaCl_2(aq) + 2H_2O(l)
The given enthalpy change (ΔH\Delta H) for this reaction is −118-118 kJ, which means that when 2 moles of HCl react completely, 118 kJ of heat is released.
Step 1: Determine the Moles of HCl
We are given 36.5 grams of HCl. The molar mass of HCl is: Molar mass of HCl=1+35.5=36.5 g/mol\text{Molar mass of HCl} = 1 + 35.5 = 36.5 \text{ g/mol}
Thus, the number of moles of HCl present in 36.5 g is: Moles of HCl=Mass of HClMolar mass of HCl=36.536.5=1 mole\text{Moles of HCl} = \frac{\text{Mass of HCl}}{\text{Molar mass of HCl}} = \frac{36.5}{36.5} = 1 \text{ mole}
Step 2: Calculate the Heat Released
From the equation, 2 moles of HCl release 118 kJ of heat. So, for 1 mole of HCl, the heat released is: Heat released=(12×(−118))=−59.0 kJ\text{Heat released} = \left(\frac{1}{2} \times (-118)\right) = -59.0 \text{ kJ}
Final Answer:
The heat released when 36.5 g of HCl reacts completely is -59.0 kJ (negative sign indicates exothermic reaction).
Now, I’ll generate an image illustrating this reaction and energy release.
Here is an illustration of the reaction between hydrochloric acid (HCl) and barium hydroxide (Ba(OH)₂), showing the mixing process, product formation, and heat release (-59.0 kJ). Let me know if you need any modifications!