Charles’s Law Experiment #JayChem
Summary
TLDRThis video script details a Charles' Law experiment, demonstrating the relationship between gas volume and temperature. A flask filled with air is heated in boiling water at 100°C (373.15 K), then inverted in cold water at 23°C. As the gas cools, it contracts, drawing water into the flask. The initial volume of gas is measured as 138 mL, and after cooling, the volume decreases to 111.5 mL, illustrating Charles' Law: volume is directly proportional to temperature when pressure is constant.
Takeaways
- 🔍 The experiment demonstrates Charles' Law, which relates the volume of a gas to its temperature.
- 🌡️ The initial temperature of the gas in the flask is set to 100 degrees Celsius (372 Kelvin), simulating boiling water conditions.
- 💧 The flask is inverted in cold water at 23 degrees Celsius to observe the effect of temperature decrease on gas volume.
- 📉 As the gas cools, its volume decreases, causing water to be drawn into the flask.
- 📏 The volume of water that enters the flask is measured to be 26.5 milliliters, representing the reduction in gas volume.
- 🔄 The initial volume of gas in the flask is assumed to be the full volume of the flask, which is 138 milliliters.
- ➖ To find the new volume of the gas after cooling (V2), subtract the volume of water drawn in from the initial volume (V1).
- 📐 V2 is calculated to be approximately 111.5 milliliters, indicating the volume change due to temperature decrease.
- 🔄 Charles' Law states that the ratio of initial volume to initial temperature should equal the ratio of final volume to final temperature.
- 📝 The experiment aims to verify Charles' Law by comparing the calculated V2 with the observed V2 from the data collection.
Q & A
What is the purpose of the Charles Law experiment described in the transcript?
-The purpose of the experiment is to observe the relationship between the volume of a gas and its temperature, as described by Charles' Law, which states that the volume of a gas is directly proportional to its temperature when pressure is held constant.
What is the initial temperature (T1) of the gas inside the flask when it is placed in boiling water?
-The initial temperature (T1) of the gas inside the flask is 100 degrees Celsius, which is also converted to Kelvin for the experiment.
How is the temperature converted from Celsius to Kelvin?
-The temperature in Kelvin is equal to the temperature in Celsius plus 273.15. So, 100 degrees Celsius is equal to 373.15 Kelvin.
What happens to the gas volume when the flask is placed in cold water?
-When the flask is placed in cold water, the gas inside cools down and contracts, leading to a decrease in volume, which causes water to be drawn into the flask.
What is the temperature of the cold water bath and how is it recorded?
-The temperature of the cold water bath is 23 degrees Celsius, and this is recorded as the second data point for temperature in the experiment.
Why does water rush into the flask when it is inverted in the cold water?
-Water rushes into the flask because the gas inside contracts as it cools, creating a vacuum that allows water to be drawn in due to atmospheric pressure.
How is the volume of the gas that has cooled and contracted measured?
-The volume of the cooled gas is measured indirectly by subtracting the volume of water that has been sucked into the flask from the total volume of the flask when it was full of hot gas.
What is the volume of water that is sucked into the flask when it is inverted in the cold water?
-The volume of water that is sucked into the flask is 26.5 milliliters.
What is the initial volume (V1) of the hot air in the flask before it is inverted in the water?
-The initial volume (V1) of the hot air in the flask is 138 milliliters, as measured by pouring the contents of the flask into a graduated cylinder.
How is the final volume (V2) of the gas calculated?
-The final volume (V2) of the gas is calculated by subtracting the volume of water sucked into the flask (26.5 milliliters) from the initial volume of the hot air (138 milliliters), resulting in approximately 111.5 milliliters.
What does Charles' Law state about the relationship between the volume and temperature of a gas?
-Charles' Law states that for a given mass of gas at constant pressure, the volume of the gas is directly proportional to its thermodynamic temperature (measured in Kelvin).
How is the validity of Charles' Law tested in this experiment?
-The validity of Charles' Law is tested by comparing the calculated final volume (V2) based on the initial volume (V1) and temperature change with the actual measured final volume (V2) from the experiment.
Outlines
🔬 Charles Law Experiment Overview
This paragraph introduces a science experiment designed to explore Charles Law, which examines the relationship between the volume of a gas and its temperature. The experiment involves heating an Erlenmeyer flask in boiling water to 100 degrees Celsius, then inverting it into cold water at 23 degrees Celsius. The goal is to observe how the gas volume changes as the temperature decreases. The initial temperature of the gas is equated to the boiling water temperature and converted to Kelvin. The experiment records the volume of water that enters the flask as the gas cools and contracts, which is used to calculate the new volume of the gas. The process includes ensuring atmospheric pressure consistency and accurately measuring the volume of water displaced by the gas contraction.
📊 Analyzing Charles Law Data
This paragraph delves into the data analysis phase of the Charles Law experiment. It explains the process of calculating the final volume of the gas (V2) after cooling by subtracting the volume of water that entered the flask from the initial volume (V1) of the hot gas. The paragraph discusses the conceptual understanding behind the experiment, emphasizing how the gas particles lose energy and contract as the temperature drops. The experiment aims to verify Charles Law, which states that the initial volume of a gas divided by its initial temperature should be proportional to the final volume divided by the final temperature. The paragraph concludes with a call to action to complete the experiment's write-up and encourages the viewer to embrace their inner science enthusiast.
Mindmap
Keywords
💡Charles Law
💡Flask
💡Boiling Water
💡Temperature
💡Volume
💡Erlenmeyer Flask
💡Cold Water Bath
💡Pressure
💡Kelvin
💡Data Points
💡Graduated Cylinder
Highlights
Charles Law experiment using a flask in boiling water to observe the relationship between gas volume and temperature.
Initial temperature (T1) set at 100 degrees Celsius, converted to Kelvin.
Placing the flask upside down in cold water causes water to rush in as the gas volume decreases.
The gas inside the flask shrinks when the temperature decreases.
The volume of water sucked into the flask is measured to be 26.5 milliliters.
The total volume of gas in the hot flask before inversion is assumed to be 138 milliliters.
V2 is calculated by subtracting the volume of water sucked into the flask from the initial volume (V1).
V2 is found to be approximately 111.5 milliliters after the subtraction.
The experiment demonstrates Charles Law, which states that the initial volume to initial temperature ratio should be proportional to the final volume to final temperature ratio.
The experiment shows that when the temperature of a gas decreases, its volume also decreases.
The relationship between volume and temperature is explored through Charles Law.
The experiment involves heating a flask in boiling water and then cooling it in cold water.
The gas particles inside the flask gain energy when heated, causing the gas to fill the entire volume of the flask.
Cooling the gas causes it to shrink, allowing water to fill the now-vacant space in the flask.
The experiment indirectly measures the volume of the colder gas by subtracting the water volume from the initial gas volume.
The experiment aims to verify Charles Law by comparing calculated V2 with the observed V2.
The lab concludes with a discussion on the observed changes in gas volume with temperature.
Transcripts
this is going to be our charles law
experiment
and first off we're going to be using a
flask in boiling water
we're basically going to be checking as
the temperature of a gas decreases
what happens to the volume of that gas
we know there's a relationship between
volume and temperature
and we like to look at that through the
eyes
of charles law today we are going to be
focused on
just the smaller flask
our first step then is going to be to
take boiling hot water
and put our erlenmeyer flask into the
hot
boiling water as the boiling water
surrounds the flask it's going to heat
the air inside the flask as well to the
same temperature
so we know that whatever temperature
that water is
that is going to be the temperature of
the gas inside
so for our first amount of temperature
t1 it's going to be 100 degrees
celsius so on your lab for the
temperature of the boiling water bath
put it 100 degrees celsius and also
convert it to kelvin
now remember that kelvin temperature in
that is actually the temperature of the
gas
initially we're then going to plug the
top of that gas
and put it upside down in cold water
and imagine what's happening there's
water that's actually going
inside this erlenmeyer flask right now
why
because the gas that was filling up that
entire flask
is now shrinking
so for your second data point you are
going to put
23 degrees celsius for the temperature
of your cold
water bath now eventually if we leave
this long enough
the gas that is inside
this erlenmeyer flask should be the same
temperature
as this cold water bath now the big
question is
why did water rush in well remember if
we dropped the temperature
that gas that was originally taking up
all of the erlenmeyer flask is now
shrinking because it's getting colder
and now where there's no gas
water will rush in so let's move forward
in the lab
now if you notice we're going to take
our hand and we're going to put the
level that the
water's at inside the flask and put it
to the same level as the top of the
water
inside the beaker the reason for that is
the outside atmospheric pressure
will be the same as the inside pressure
we'll then plug it and pull it out of
the water so we don't lose any of the
water
inside the flask now if you think about
it
the water inside that flask is the
volume
that the gas shrunk so let's measure
that volume of water that's inside the
flask and sucked into it
and that is by the way going to be a
data point
the volume of water sucked into the
flask
so there you have it it's going to be
26.5 milliliters for the volume of water
sucked into the flask
go ahead and put those milliliters into
your data table so that you have that
and then let's move forward so we can
eventually figure out
what's the total volume of the gas that
was in the
hot erlenmeyer flask before it was
inverted in the water
so let's go ahead and do that
i'm going to fill up our erlenmeyer
flask
all the way
because that's how much volume the gas
would have been
when your erlenmeyer flask was
completely full
now we're going to take that and pour it
into the graduated cylinder
and this is going to give us the assumed
volume of the hot air in the flask
technically our v1
as you can see the volume of the hot air
assumed in the flask is going to be 138
milliliters
go ahead and put that for your v1 data
point
and make sure that's in milliliters
so here we're going to take a look at
how do we figure out how much
volume of gas was when it was cooled
so what we're saying is we're trying to
find our
v2 reading to do that
our v2 reading we're going to take the
total volume
v1 the starting volume of the hot air
and we subtract
the amount of water that was sucked into
the flask
when you subtract that you end up
getting
about 111.5 milliliters
and that'll be your official v2 the
other way to find that if you look on
your data table is to take the data from
d and subtract letter data c
from it as well and that's just what we
did
let's think about what's really
happening in this lab to start with
you have this erlenmeyer flask that is
heating up in the boiling water so
inside this flask all these little
particles of gas
are getting the same amount of energy as
the water outside
so we know that when this gas is heated
up to the same temperature of the
boiling water
right that this gas is completely
filling the entire volume of the flask
and it's at that same temperature but
once we
cool down that gas and invert it upside
down
you notice that there was water that
filled up that flask
what does that mean well what happened
was the gas used to fill up the entire
flask
but now that the water was colder
the gas got colder and it shrunk a
little bit
so what we have to do is we have to take
the entire
volume of this flask and subtract out
the small amount of water and when you
subtract that out
that becomes the new volume of the cold
gas
so that's what we did we measured
indirectly
how much water that erlenmeyer flask
sucked in
and by knowing that however much water
took the place of gas
if we subtract that out we now have our
new volume of the colder gas
so just so you know that's why we did
that subtraction problem
now when we're looking at that think
about everything that's happening with
charles law
here is our data we started 100 degrees
that was our hot gas and we ended
with the 23 degrees or so now that you
have that
we've seen charles law in action
remember charles law is the initial
volume
over the initial temperature should be
proportional
to the final volume over the final
temperature
the question is though was this holding
true
so you are going to use your data to
basically
solve for what v2 would have been
according to the math
and see how closely related it was
to the v2 that you got in data
collection
letter e and we're going to compare
those
but remember charles law shows that
relationship between volume and
temperature
so the question is once again if we drop
the temperature
of a gas what happens to the volume of
the gas
did it go up or did it go down
that is our main goal of this lab so now
that you have that data
go ahead and finish your write up for
charles law be well science fan
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