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Cold packs, whose temperatures are lowered when ammonium nitrate dissolves in water, are carried by athletic trainers when transporting ice is not possible. Which of the following is true of this reaction?

a. ΔH < 0, process is exothermic
b. ΔH > 0, process is exothermic
c. ΔH < 0, process is endothermic
d. ΔH > 0, process is endothermic
e. ΔH = 0, since cold packs are sealed

Sagot :

dsdrajlin

Answer:

d. ΔH° > 0, process is endothermic.

Explanation:

Cold packs contain ammonium nitrate (NH₄NO₃). When this salt dissolves in water, it decreases the temperature of the surroundings. This happens because the process is endothermic (absorbs heat from the surroundings). By convention, when a process is endothermic, the standard enthalpy carries a positive sign (ΔH° > 0).

The process is endothermic (ΔH > 0) when cold packs, whose temperatures are lowered when ammonium nitrate dissolves in water, are carried by athletic trainers when transporting ice is not possible.

What is an endothermic reaction?

Endothermic reactions is a chemical reactions that involves the reactants absorbing heat energy from the surroundings.

Here, the products energy increase while the surrounding temperature will reduce.

  • When this Ammonium nitrate dissolves in water, temperature of the surroundings reduces and the and the endothermic standard enthalpy carries a positive sign (ΔH° > 0).

Therefore, the process is endothermic (ΔH > 0) when cold packs, whose temperatures are lowered when ammonium nitrate dissolves in water, are carried by athletic trainers when transporting ice is not possible.

For more details on endothermic reaction kindly check

https://brainly.com/question/1447631

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