Cool a Drink in 2 Minutes

52,607

383

40

Introduction: Cool a Drink in 2 Minutes

How to cool down a can of drink in 2 minutes. A simple science trick to give you a speedy ice cold beverage which won't get diluted like it would if you were to put ice cubes in your drink. Perfect for cooling beer and soda cans in an emergency, and you can even use it for chilling wine bottles.

Step 1: Getting Started

What you need:

  • A can of drink
  • A bowl
  • Ice cubes
  • Salt
  • A spoon
  • A thermometer (optional)

When you have everything you need, go ahead and follow the instructions or watch the video for a visual demonstration and full instructions.

Step 2: Set Up

Take your bowl fill it with water until its roughly one third full. Then take some ice cubes from the freezer and tip them into the bowl. I used two trays of ice cubes.

Step 3: Chemical Reaction

Next add a couple of table spoons of salt into the ice water and stir it in. As the salt dissolves into the water, it will actually disassociate into its constituent, sodium and chloride ions. Water molecules are polar, and each molecule has a partially positive and a partially negative charged end. The negative end attracts the positive sodium ion, and the positive end attracts the negative end. This process (known as solvation) requires energy which is obtained by reducing the thermal energy of the water, hence reducing the temperature of the salt ice-water mix. The ice will not only melt, but actually get colder!

Step 4: Cooling the Drink

Once you've stirred in the salt, carefully place your drink into the solution and submerge it.

As the salt ice-water solution is so much colder then the room temperature drink, the heat energy in the can will be drawn out and the temperature of the drink inside the can will rapidly reduce.

Second law of thermodynamics states: Two substances with different temperatures reach thermal equilibrium over time.

After a minute give it all a good stir with a spoon and after 2 minutes its ready to take out. The temperature of your drink will have reduced significantly, and you can now enjoy a nice cold ice cold drink!

Step 5: Measure the Change

If you like you can monitor the temperature change by checking the temperature of a room temperature can, and comparing it to the temperature of a can after its been cooled in the solution. I left the can in the solution for 2 minutes and found the temperature fell from 75°F (24°C) to 41°F (5°C) which is a reduction in temperature of 34°F or 19°C.

This science is not only a fun and practical way to quickly cool down your drink, but it can also be used for making home made ice-cream.

Explore Science Contest

Participated in the
Explore Science Contest

Be the First to Share

    Recommendations

    • Candy Speed Challenge

      Candy Speed Challenge
    • The 1000th Contest

      The 1000th Contest
    • Battery Powered Contest

      Battery Powered Contest

    40 Discussions

    0
    ViCe CriSpYy
    ViCe CriSpYy

    2 years ago

    Or we could just put in some ice...

    0
    stephenmack
    stephenmack

    5 years ago on Introduction

    I love doing this because of how much the salt speeds the process up!

    0
    maniacse
    maniacse

    Reply 5 years ago on Introduction

    I just dont get reason of this ible, but then I read whole instructions, and as you mentioned, the rise of speed due using of salt is just perfect! Just basic knowledge put together and here we go.. Thanks to autor for this ible!

    0
    Zendo_Xarth
    Zendo_Xarth

    5 years ago on Introduction

    What would have been neat is if you did the same thing in another bowl but did not use the salt to find out how much the salt helped cool the drink.

    But still really cool.

    0
    Anderson_Lim_Mys
    Anderson_Lim_Mys

    Reply 5 years ago on Introduction

    gthompson20 is right. Though dissociation of salt does happen, but what actually make the salt water cooler is the ices absorb heat from surroundings in order to melt because its freezing point have reduced. The latent heat of melting of ice is HUGE compared to heat of dissociation of sodium chloride.

    0
    gthompson20
    gthompson20

    Reply 5 years ago on Introduction

    That is absolute rubbish about the sodium and chlorine dissociating. They do no such thing the salt is just dissolved in the water turning it into salt water which has a freezing point of 0 deg F when the temp of the ice can be as high as 32 deg F

    Since it has now been turned into salt water the latent heat of the fusion of the ice has to be replaced and it is absorbed from the surrounds. If my memory serves me right, from high school physics, this is how 0 deg F was originally defined

    The same mechanism can be used to actually freeze pure water if isolated from the salt.

    0
    introvertedone
    introvertedone

    Reply 5 years ago

    Dissociation of salt: https://youtu.be/EBfGcTAJF4o

    0
    MultaeKappae
    MultaeKappae

    Reply 5 years ago on Introduction

    Good link.

    The salt dissociation is neither an endothermic or exothermic reaction (it's a mechanical change, not a chemical one).
    http://antoine.frostburg.edu/chem/senese/101/solut...

    http://hyperphysics.phy-astr.gsu.edu/hbase/thermo/...

    TL;DR : it 'costs' heat to melt ice. Since salt water freezes at a lower temperature, the now cooler salt water isn't starting to freeze in response to losing heat, so the heat exchange is faster, which means there is less time to absorb ambient heat from outside the system.

    ...in short, everyone is right.
    kinda

    0
    xmac1x
    xmac1x

    Reply 5 years ago on Introduction

    You are mistaken. Sodium chloride does dissociate in water, hence why it is used to make electrolyte solutions. The ions are free to carry charges in the aqueous phase

    0
    discostu956
    discostu956

    Reply 5 years ago

    it's pretty well known that sodium chloride dissociates when it's dissolved in water.

    0
    gthompson20
    gthompson20

    Reply 5 years ago on Introduction

    Well it looks like my chemistry teacher was telly me a load of BS. It doesn't change the fact that 50 years ago this method was used in toy ice cream makers to obtain sub zero C temperatures, it is just rehashing what most people already know

    0
    bbabin
    bbabin

    Reply 5 years ago on Introduction

    And exactly how many Instructables have you contributed??? Right. That's what I thought. Honestly, there are more constructive ways to approach the apparent issue you have with this experiment. Please see the "be nice" comment policy shown every time you comment on others work.

    0
    thundrepance
    thundrepance

    Reply 5 years ago on Introduction

    ditto. i look thru these for cool, fun ideas [like this one]. if i don't care for one, i simply move on.

    it really doesn't make people heroes in the eyes of others to look thru these "instructibles" {how i think it should be spelled x^)} & bully nice folks, gt20.

    0
    laughingmoonx

    And it used to make the BEST ice cream in the world! Who cares how, if it works, it works!

    0
    szczech926
    szczech926

    5 years ago on Introduction

    I find it works much quicker and cheaper by putting the drink into a glass and then the ice cubes into the glass

    0
    hmuckleroy
    hmuckleroy

    5 years ago on Introduction

    I always just put it in the microwave and set the timer to a negative number.

    0
    DIY-Guy
    DIY-Guy

    Reply 5 years ago on Introduction

    HMuckleroy, Nice... negative numbers on the microwave timer.
    Or, just set any timer to a negative number and let time run backwards until it's cool when you pull it out to drink.

    0
    DavidS40
    DavidS40

    Reply 5 years ago on Introduction

    I can't believe I didn't think of this.