**Calorimetry Experiment: Determining ΔH for LiOH Dissolution**In a calorimetric experiment, 6.48 grams of lithium hydroxide (LiOH) was dissolved in water. This caused the temperature of the calorimeter to increase from 25.00°C to 36.66°C. The task is to determine the enthalpy change (ΔH) for the solution process.**Chemical Reaction:**\[ \text{LiOH}_{(s)} \rightarrow \text{Li}^{+}_{(aq)} + \text{OH}^{-}_{(aq)} \]**Heat Capacity:**The combined heat capacity of the calorimeter and its contents is 547 J/°C.---**Calculating ΔH:**To find ΔH, we need to calculate the heat absorbed or released using the formula:\[ q = C \times \Delta T \]Where:- \( q \) is the heat absorbed or released,- \( C \) is the heat capacity,- \( \Delta T \) is the change in temperature.\[ \Delta T = 36.66°C - 25.00°C = 11.66°C \]\[ q = 547 \, \text{J/°C} \times 11.66 \, \text{°C} \] Calculate \( q \) to find the enthalpy change, considering the mass of the solute and stoichiometry of the reaction.

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6.111 In a calorimetric experiment, 6.48 g of lithium hy- droxide, LİOH, was dissolved in water. The temperature of the calorimeter rose from 25.00°C to 36.66°C. What is AH for the solution process? LIOH(s) → Li*(aq) + OH(aq) The heat capacity of the calorimeter and its contents is 547 J/°C.

6.111 In a calorimetric experiment, 6.48 g of lithium hy- droxide, LİOH, was dissolved in water. The temperature of the calorimeter rose from 25.00°C to 36.66°C. What is AH for the solution process? LIOH(s) → Li*(aq) + OH(aq) The heat capacity of the calorimeter and its contents is 547 J/°C.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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