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In a coffee cup calorimeter, 100.0 mL of 1.0 M NaOH and
Chapter 9, Problem 9.55(choose chapter or problem)
In a coffee cup calorimeter, 100.0 mL of 1.0 M NaOH and 100.0 mL of 1.0 M HCl are mixed. Both solutions were originally at \(24.6^{\circ} \mathrm{C}\). After the reaction, the final temperature is \(31.3^{\circ} \mathrm{C}\). Assuming that all the solutions have a density of \(1.0 \mathrm{~g} / \mathrm{cm}^{3}\) and a specific heat capacity of \(4.18 \mathrm{~J}^{\circ} \mathrm{C}^{-1} \mathrm{~g}^{-1}\), calculate the enthalpy change for the neutralization of HCl by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter.
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QUESTION:
In a coffee cup calorimeter, 100.0 mL of 1.0 M NaOH and 100.0 mL of 1.0 M HCl are mixed. Both solutions were originally at \(24.6^{\circ} \mathrm{C}\). After the reaction, the final temperature is \(31.3^{\circ} \mathrm{C}\). Assuming that all the solutions have a density of \(1.0 \mathrm{~g} / \mathrm{cm}^{3}\) and a specific heat capacity of \(4.18 \mathrm{~J}^{\circ} \mathrm{C}^{-1} \mathrm{~g}^{-1}\), calculate the enthalpy change for the neutralization of HCl by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter.
ANSWER:Step 1 of 3
Enthalpy change indicates the energy lost/gained during a specific process. It also represents the heat content in a specific system. It can be denoted using the letter q.