# Why is freezing an exothermic process?

Reema

In this process of freezing, water loses heat to the surroundings, so it is an exothermic process.

Solidifying is a procedure of fluid changing its state to strong. How about we investigate the procedure intently. We should begin with water. Some water contains a lot of modest H2O particles. Each little atom is moving and has some measure of vitality. At the point when the water is put in a cooler, the water gradually loses warmth to the encompassing virus air. The water particles on losing vitality start to move gradually, come nearer and pack close enough to change to ice.

In this procedure, the water discharges warmth to the environment, so it is an exothermic procedure. At the point when water lose vitality, the individual atoms move slower (diminished dynamic vitality). In the end the water atoms will move toward becoming secured (solidify) as they augment the quantity of hydrogen bonds they structure with other water particles.

Example1:

Does freezing release energy?

At the point when water solidifies it surrenders a portion of the water's vitality. This vitality that is surrendered is the dormant warmth of solidifying. At the point when the water was frigid dormant warmth of solidifying vitality was being discharged. Vitality is being exchanged even through the temperature is steady.

Example2:

Why is making ice cubes exothermic?

At the point when water is solidified into ice 3D shapes, heat is emitted to the environment. This makesthe solidifying of ice an exothermic response. As the water cools, and after that solidifies, it starts to move increasingly more gradually as it turns into a strong. Amid that procedure, that vitality is discharged as warmth.

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Related Questions
##### 2. (11 marks) a) At 400 Â°C, ammonium iodide decomposes in the following endothermic reaction: NH41(s) + NH3(g) + HI(g) Kp = 0.215 at 400 Â°C. Write the equilibrium expression for this reaction. 15.0 g of NH4I was placed in an empty 3.0 L flask and heated to 400 Â°C. What is the partial pressure of NH3 in the flask once the reaction has reached equilibrium? How would the following changes to the equilibrium mixture affect the number of moles of NH3 in the flask and the value of K, once equilibrium is re-established? (Use increase, decrease or stay the same.) Change Effect on moles of NH3 Ke value Increase temperature Increase volume of flask Remove half of HI gas
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