Chem Stoichiometry April Test - concepts

Which gas laws show direct relationships?

Avogadro's & Gay-Lussac's (V-n and P-T)

Why can gases take the shape of any container?

Expansion (particles spread out to fill space)

Gas escaping through a tiny hole

Effusion

What does Kinetic Molecular Theory explain?

Gas behavior based on particle motion & energy

Which gases behave most ideally?

Small, nonpolar gases (ex: He)

Which gas diffuses slowest?

Largest molar mass gas

When do gases behave most ideally?

High temperature & low pressure

-173°C in Kelvin

100 K

Pressure ↑, volume ↓ (constant temp)

Boyle's Law

At same temperature, all gases have same what?

Average kinetic energy

Gas particles spacing (KMT)

Very far apart

Attractive forces in gases (KMT)

None/negligible

Type of collisions in gases

Elastic (no energy lost)

What causes gas pressure?

Collisions with container walls

What determines kinetic energy?

Temperature only

Standard pressure

1 atm = 760 mmHg

Volume of 1 mole at STP

22.4 L

When do gases deviate from ideal behavior?

Low temp & high pressure

Dalton's Law

Total pressure = sum of partial pressures

Ideal Gas Law

PV = nRT

Value of R (atm units)

0.0821 L·atm/mol·K

Type of collision with no energy loss

Elastic collision

Most abundant gas in atmosphere

Nitrogen

Which gas is more ideal: H2 or NH3?

H2 (smaller & nonpolar)