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A quantity of 2.00 × 102 mL of 0.862 M HC1 is mixed with
Chapter 6, Problem 77P(choose chapter or problem)
A quantity of \(2.00 \times 10^{2}\ \mathrm{mL}\) of 0.862 M HCl is mixed with an equal volume of \(0.431\ M\ B a(O H)_{2}\) in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of the HCl and \(B a(O H)_{2}\) solutions is the same at \(20.48^{\circ} \mathrm{C}\), For the process
\(H^{+}(a q)+O H^{-}(a q) \rightarrow H_{2} O(l)\)
the heat of neutralization is - 56.2 kJ/mol. What is the final temperature of the mixed solution?
Questions & Answers
QUESTION:
A quantity of \(2.00 \times 10^{2}\ \mathrm{mL}\) of 0.862 M HCl is mixed with an equal volume of \(0.431\ M\ B a(O H)_{2}\) in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of the HCl and \(B a(O H)_{2}\) solutions is the same at \(20.48^{\circ} \mathrm{C}\), For the process
\(H^{+}(a q)+O H^{-}(a q) \rightarrow H_{2} O(l)\)
the heat of neutralization is - 56.2 kJ/mol. What is the final temperature of the mixed solution?
ANSWER:Step 1 of 2
Here, we are going to calculate the final temperature of the mixed solution.
We know that,
-
The heat produced by the reaction is given below:
= -9.69 kJ
Thus,
Heat produced by the reaction