Application
What is one real-world use of Avogadro’s Law in safety devices?
Ex answer - Car airbags fill rapidly due to gas molecules expanding in volume.
State Avogadro’s Law
At constant temperature and pressure, volume is directly proportional to the number of moles
Calculate the volume if 0.119 mol of gas occupies 1.2 L and the moles increase to 0.274 mol.
2.8 L (using V1/n1 = V2/n2).
What does Avogadro’s Law say about equal volumes of gases?
They contain equal numbers of molecules at the same temperature and pressure.
Why are gases considered fluids?
Because they flow and take the shape of their containers.
How does Avogadro’s Law help in gas storage and transportation?
It helps engineers determine how many moles of gas fit in a container at constant temperature and pressure.
What does the formula V1/n1 = V2/n2 represent?
It shows the relationship of volumes and moles between two gasses, assuming constant temperature and pressure.
Given 4 moles in 12 L, find moles in 30 L container.
10 moles (using V1/n1 = V2/n2).
Who was Avogadro and what did he contribute?
A scientist who proposed that equal volumes of gases contain equal numbers of molecules.
How does temperature affect gas volume
Volume increases with temperature if pressure and moles stay constant.
Describe how your lungs demonstrate Avogadro’s Law during breathing.
When inhaling, more gas molecules enter, increasing lung volume; when exhaling, volume decreases as molecules leave.
How does Avogadro’s Law support the idea that chemical reactions involving gases can be predicted using volume ratios?
Avogadro’s Law shows that equal volumes of gases at the same temperature and pressure contain equal numbers of particles. This allows them to use volume ratios of reactants and products in gas reactions (like using mole ratios in stoichiometry)
A container has 37 grams of C₂Te₄ gas, which fills 22.4 liters. If 16.8 liters of the gas is removed, how much gas (in grams) is left?
(Hint: The mass can be converted to moles)
9.25 g.
How is Avogadro’s Law useful in chemistry labs?
It helps predict volumes of gases involved in reactions.
How does temperature affect gas volume according to gas laws?
Volume increases with temperature if pressure and moles stay constant.
How does a bicycle pump demonstrate Avogadro’s Law? ( Hint what happens to volume and pressure )
Pumping air increases the number of gas molecules inside the tire, which increases the tire’s volume and pressure.
Why is it important to keep temperature and pressure constant when using Avogadro’s Law?
Because Avogadro’s Law only works when temperature and pressure stay the same. If they change, volume can change for other reasons, and the number of gas particles (moles) won’t be the only factor affecting volume.
A flat ball contains 3.5 moles of gas and occupies a volume of 7.0 liters at constant temperature and pressure. If the gas is added until the volume increases to 10.5 liters, how many moles of gas are in the ball now.
(Hint: n2=V1V2×n1)
5.25mol
Why must temperature and pressure be constant in Avogadro’s Law?
Because volume depends on these variables too; changing them affects gas behavior.
Explain how intermolecular forces affect gas properties.
Weak forces mean the gases can spread out easily, but stronger forces mean the gas particles are closer meaning, which can cause condensation.
Explain how Avogadro’s Law is important for ensuring maximum efficiency in industrial gas container design. (Hint - what does it help containers do)
It allows precise calculation of gas quantity and volume so containers are filled safely without leaks or overpressure.
Explain why Avogadro’s Law is important when doing stoichiometry with gases in a chemical reaction.
Avogadro’s Law lets you treat gas volume like moles when temperature and pressure are constant. That means you can use volume ratios instead of just mole ratios to solve problems faster.
Hydrogen, Fluorine, and Chlorine gases occupy 100g combined. Calculate which gas occupies the largest volume using molar masses and mole calculations.
Hydrogen gas occupies the largest volume.
Why don’t real gases always follow the ideal gas rules? How do things like pressure and temperature affect this?
( Hint: real gases are gases in the real world, like oxygen, nitrogen, carbon dioxide, and helium )
Real gases don’t always follow the rules because their particles can stick together a little (intermolecular forces) and take up space. At high pressure, the gas gets squeezed, so the particles are closer together. At low temperature, the particles move slower, so they stick more. This makes real gases act differently than ideal gases.
What makes real gases different from ideal gases?
Real gases have particles that take up space and can attract each other a little. That makes them act differently, especially when they’re cold or squeezed under high pressure. (real gases don’t always behave exactly as the gas laws predict)