The final temperature of the instant hot pack contain a solid and a pouch of water have to determine. Concept introduction: The amount of heat required to change the temperature of a substance taking part in any reaction or phase transition is the fundamental theme of the calorimetric problems. Given: Instant hot packs contain a solid and a pouch of water, when the pack is squeezed, the pouch breaks and the solid dissolves, increasing the temperature due to the exothermic reaction. The following reaction is used to make a hot pack L i C l ( s ) → H 2 O L i + ( a q ) + C l − ( a q ) Δ H = -36 .9 k J . 25.0g of LiCl dissolved in 125 mL of water. The initial temperature is 25 o C and the specific heat of the solution is 4.18 J/ (g. o C). No heat transfer between the hot pack and the environment. To determine: The amount of heat required to change of the reaction involve in hot pack.

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Chapter 9, Problem 9.79SP

Interpretation Introduction

Interpretation:

The final temperature of the instant hot pack contain a solid and a pouch of water have to determine.

Concept introduction:

The amount of heat required to change the temperature of a substance taking part in any reaction or phase transition is the fundamental theme of the calorimetric problems.

Given: Instant hot packs contain a solid and a pouch of water, when the pack is squeezed, the pouch breaks and the solid dissolves, increasing the temperature due to the exothermic reaction. The following reaction is used to make a hot pack LiCl(s)→H2OLi+(aq)+Cl−(aq) ΔH= -36.9 kJ. 25.0g of LiCl dissolved in 125 mL of water. The initial temperature is 25 ^oC and the specific heat of the solution is 4.18 J/ (g. ^oC). No heat transfer between the hot pack and the environment.

To determine:

The amount of heat required to change of the reaction involve in hot pack.

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