University:
Eastern Kentucky University
Course:
CHE 111 | General Chemistry
Academic year:

2020
Views:

276

Pages:

1
Author:

Amira Hester

General Chemistry 8: The Gas Phase Ideal Gases Real Gases Ideal Gas: Theoretical gas whose molecules occupy negligible space and whose collisions are perfectly elastic. Gases behave ideally under reasonably !temperatures and ¯pressures. STP: 273 K (0°C), 1 atm 1 mol Gas: At STP 1 mol of gas = 22.4 L Units: 1"atm = 760"mmHg = 760"torr = 101.3"kPa = 14.7"psi Real gases deviate from ideal behavior at ¯temperature & !pressure At Moderately ! P, ¯ V, Real gases will occupy less volume than or ¯ T: predicted by the ideal gas law because the particles have intermolecular attractions. At Extremely ! P, ¯ V, Real gases will occupy more volume than or ¯ T: predicted by the ideal gas law because the particles occupy physical space. 𝑛T 𝑎 Van der Waals d𝑃 + " T j (𝑉 − 𝑛𝑏) = "𝑛R𝑇 𝑉 Equation of State: a corrects for attractive forces b corrects for volume of the particles themselves Ideal Gas Law 𝑷"𝑽 = 𝒏"𝐑"𝑻 Density of Gas: r = DH CH Combined Gas Law: GH B C R = 8.314" = Kinetic Molecular Theory FG D CI = GI (n is constant) I H L C L L = k or CH = CI H (T and P are constant) I Boyle’s Law: PV = k or P1V1 = P2V2 Charles’s Law: Avg Kinetic𝐾𝐸 = " S "𝑚"𝑣T = " W "𝐾X "𝑇 T T Energy of a Gas: (𝐾𝐸" ∝ 𝑇) G DH I ) V2 = V1D( )"( G I Avogadro’s Principle: = >?@"A DE C G = k or D CH CI = GH GI D D H I Gay-Lussac’s Law: G = k or GH = GI (n and T are constant (n and P are constant) (n and V are constant) 𝐾X = 1.38" ×" 10[TW "A !T = molecules move FASTER !molar mass = molecules move SLOWER Root-Mean3R𝑇 Square Speed: 𝑢^>_= " ` 𝑀 Diffusion: The spreading out of particles from [high] ® [low] Effusion: The mvmt of gas from one compartment to another through a small opening under pressure Other Gas Laws Graham’s Law: bH bI EI EH ¯molar mass = diffuse/effuse FASTER !molar mass = diffuse/effuse SLOWER Dalton’s Law: PT = PA + PB + PC + … (total pressure from partial pressures) Dalton’s Law: PA = XAPT =c (X = mol fraction) (partial pressure from total pressure) [P]H Henry’s Law: [A] = kH x PA or DH = [P]I DI = kH Diatomic Gases Exist as diatomic molecules, never a stand-alone atom. Includes H2, N2, O2, F2, Cl2, Br2, and I2 Mnemonic: “Have No Fear Of Ice Cold Beer” The 7 Diatomic Gases =