charmaine sy sabado

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**chemistry project**

IDEAL GAS LAW

is a single expression combining Boyle's Law, Charles' Law and Avogadro's Law.

The ideal gas law is the most important gas law for you to know: it combines all of the laws you learned about in this chapter thus far, under a set of standard conditions.

Ideal Gas Law Problems

= (0.250 x 8.314 x 300) / 200

= 623.55 / 200

find the volume from the 0.250 moles gas at 200kpa and 300k temperature.

given:

P = 200 kPa,

n = 0.250 mol,

T = 300K,

R = 8.314 J

K-1

mol-1

Substitute the values in the below volume equation:

Volume(V) = nRT / P

Volume(V) = 3.12 L

Now try an example using the ideal gas law equation

1.A small amount of water is placed in this Incan. The water is heated to a vigorous boil, As the water is heated, temperature goes up, so pressure goes up.

2. In turn, moles of gas particles begin to rapidly go down to relieve this pressure by leaving out of the Incan.

4. This causes the volume to shrink dramatically.

sample problem

In 1662, Anglo-Irish physicist and chemist Robert Boyle showed his experiments how the volume of gas responded to changes in its pressure.he summarized his law observations in a statement now known as the Boyle's Law.

more than 100 years after Robert boyle conceptualized

his Boyle's Law, Jacques Charles studied the effect of temperature on the volume of a confined gas at constant pressure.His observations on the relationship of volume and temperature were generalized into a statement known today as Charles's Law

the ideal gas equation is

PV=nRT

the volume (V) occupied by n moles of any gas has a pressure (P) at temperature (T) in kelvin

3.Once the heat is removed, and the volume is sealed, the temperature begins to go down causing the pressure to go down.

Helium and an unknown gas leak from a container. Helium effuses 2.83x faster than the unknown gas. What is the unknown gas?

You have the rate, and one mass.

Rate1/Rate2 = 2.83 = Sqrt(Mass2/Mass1)

2.83 = Sqrt (Mass2/4g)

8(4g) = Mass 2

Mass2 = 32g which is probably O2.

Graham's Law of Effusion

experiment time!

what just happend?

Amadeo Avogadro - Italian mathematical physicist who showed in what became known as Avogadro’s law that, under controlled conditions of temperature and pressure, equal volumes of gases contain an equal number of molecules.

PV=nRT

pressure

volume

number of moles

gas constant

temperature

Additionally, the number of moles in the container have been greatly reduced.

The rate of effusion of a gas is inversely proportional to the square root of either the density or the molar mass of the gas.

Effusion is the process in which a gas escapes through a small hole.

v = velocity

V = volume

Graham's law, known as Graham's law of effusion, was formulated by Scottish physical chemist Thomas Graham in 1848. Graham found experimentally that

Try it yourself!

Answer.

How do we use it?

How do we use it?

Graham's law compares the rate of effusion of two gas particles. Given parts of the question, (Rate a, Rate b, Mass a, or Mass b), just plug in the values to calculate the missing variable.

solution:

What You Need:

baking soda

vinegar

plastic bottle

balloon

funnels (we used 2)

What To Do:

1. Using your funnel pour vinegar into your bottle.You only need to fill about 1/3 of the bottle.

2. Using another (dry) funnel pour baking soda into your balloon.

Fill the balloon approx. 1/2 way.

3. Cover the top of the bottle with you balloon.

Make sure you don't let the baking soda spill into the bottle prematurely.

4. When ready, lift your balloon and let the baking soda fall into the vinegar.

5. Watch as the mixture fizzes, bubbles & expands your balloon!

The science behind it :

Baking soda and the vinegar create an ACID-BASE reaction. When combined/mixed they create a gas - carbon dioxide. Gasses need room to spread, so the

carbon dioxide fills the bottle and then moves into the balloon inflating it.

group five members:

Sabado,Charmaine

Ballud,Melissa

Cangco,Rogie

Nuynuyan,Christine

Cuaresma,Gerald

Sundiam,Dustine

Agawa,Larry