Solution Found!
A quantity of 4.00 X 102mL of 0.600 M HN03 is mixed
Chapter 6, Problem 8PE(choose chapter or problem)
Practice Exercise A quantity of \(4.00 \times 10^{2}\ \mathrm{mL}\) of \(0.600\ \mathrm{M}\ \mathrm{HNO}_{3}\) is mixed with \(4.00 \times 10^{2}\ \mathrm{mL}\) of \(0.300\ \mathrm{M\ Ba}(\mathrm{OH})_{2}\) in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of both solutions is the same at \(18.46^{\circ} \mathrm{C}\). What is the final temperature of the solution? (Use the result in Example 6.8 for your calculation.)
Questions & Answers
QUESTION:
Practice Exercise A quantity of \(4.00 \times 10^{2}\ \mathrm{mL}\) of \(0.600\ \mathrm{M}\ \mathrm{HNO}_{3}\) is mixed with \(4.00 \times 10^{2}\ \mathrm{mL}\) of \(0.300\ \mathrm{M\ Ba}(\mathrm{OH})_{2}\) in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of both solutions is the same at \(18.46^{\circ} \mathrm{C}\). What is the final temperature of the solution? (Use the result in Example 6.8 for your calculation.)
ANSWER:Step 1 of 4
Heat of the solution can be calculated by the following formula;
Here,
