Instant cold packs, often used to ice athletic injuries on the field, contain ammonium nitrate and water separated by a thin plastic divider. When the divider is broken, the ammonium nitrate dissolves according to the following endothermic reaction: NH4NO3(s)→NH4+(aq)+NO3−(aq)NH4NO3(s)→NH4+(aq)+NO3−(aq) In order to measure the enthalpy change for this reaction, 1.35 gg of NH4NO3NH4NO3 is dissolved in enough water to make 20.5 mLmL of solution. The initial temperature is 24.5 ∘C∘C and the final temperature (after the solid dissolves) is 20.0 ∘C∘C. Calculate the change in enthalpy for the reaction in kJkJ. (Use 1.0gmL−11.0gmL−1 as the density of the solution and 4.184Jg−1∘C−14.184Jg−1∘C−1 as the specific heat capacity.) Express your answer to two significant figures and include the appropriate units.
Instant cold packs, often used to ice athletic injuries on the field, contain ammonium nitrate and water separated by a thin plastic divider. When the divider is broken, the ammonium nitrate dissolves according to the following endothermic reaction: NH4NO3(s)→NH4+(aq)+NO3−(aq)NH4NO3(s)→NH4+(aq)+NO3−(aq) In order to measure the enthalpy change for this reaction, 1.35 gg of NH4NO3NH4NO3 is dissolved in enough water to make 20.5 mLmL of solution. The initial temperature is 24.5 ∘C∘C and the final temperature (after the solid dissolves) is 20.0 ∘C∘C. Calculate the change in enthalpy for the reaction in kJkJ. (Use 1.0gmL−11.0gmL−1 as the density of the solution and 4.184Jg−1∘C−14.184Jg−1∘C−1 as the specific heat capacity.) Express your answer to two significant figures and include the appropriate units.
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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Instant cold packs, often used to ice athletic injuries on the field, contain ammonium nitrate and water separated by a thin plastic divider. When the divider is broken, the ammonium nitrate dissolves according to the following endothermic reaction:
In order to measure the enthalpy change for this reaction, 1.35 gg of NH4NO3NH4NO3 is dissolved in enough water to make 20.5 mLmL of solution. The initial temperature is 24.5 ∘C∘C and the final temperature (after the solid dissolves) is 20.0 ∘C∘C.
NH4NO3(s)→NH4+(aq)+NO3−(aq)NH4NO3(s)→NH4+(aq)+NO3−(aq)
In order to measure the enthalpy change for this reaction, 1.35 gg of NH4NO3NH4NO3 is dissolved in enough water to make 20.5 mLmL of solution. The initial temperature is 24.5 ∘C∘C and the final temperature (after the solid dissolves) is 20.0 ∘C∘C.
Calculate the change in enthalpy for the reaction in kJkJ. (Use 1.0gmL−11.0gmL−1 as the density of the solution and 4.184Jg−1∘C−14.184Jg−1∘C−1 as the specific heat capacity.)
Express your answer to two significant figures and include the appropriate units.
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