chemistry 161 chapter 5 chem.hawaii/bil301/welcome.html
DESCRIPTION
CHEMISTRY 161 Chapter 5 www.chem.hawaii.edu/Bil301/welcome.html. REVISION. Boyle’s Law Gay-Lussac’s Law Avogadro’s Law. p ∞ 1/V. V ∞ T. n ∞ V. 1. IDEAL GAS EQUATION. (1) p ∞ 1/V. V ∞ 1/p. (2) V ∞ T. V ∞ T. (3) n ∞ V. V ∞ n. V ∞ T × n / p. p × V = const × n × T. - PowerPoint PPT PresentationTRANSCRIPT
CHEMISTRY 161
Chapter 5
www.chem.hawaii.edu/Bil301/welcome.html
REVISIONBoyle’s Law
Gay-Lussac’s Law
Avogadro’s Law
p ∞ 1/V
n ∞ V
V ∞ T
(1) p ∞ 1/V
p × V = const × n × T
(2) V ∞ T
1. IDEAL GAS EQUATION
(3) n ∞ V
V ∞ 1/p
V ∞ T
V ∞ n
V ∞ T × n / p
p × V = const × n × T
p × V = R × n × T
p × V = n × R × T
ieal gas equation
p × V = n × R × T
[R] = [p] × [V] / [n] / [T]
Pa = N/m2 m3 mol K
[R] = N × m / mol / K
[R] = J / mol / K
R = 8.314 J / mol / K
[R] = J / mol / K
ideal gas constant
p × V = n × R × T
2. MOLAR VOLUME
What is the volume of 1 mol of a gas at
273.15 K (0oC) and 1 atm (101,325 Pa)?
standard temperature and pressure
(STP)
V = 22.4 l
p × V = n × R × T
the molar volume at standard pressure and temperature is independent on the gas type
V = 22.4 l
Vm = 22.4 l
3. STOICHIOMETRY
NaN3(s) → Na(s) + N2(g)
How many liters of nitrogen gas are produced in the decomposition of 60.0 g sodium azide at 80oC and 823 torr?
1. Balancing
2. Mole ratios
3. Convert grams into moles
4. Convert moles into liters
4. DENSITY CALCULATION
p × V = n × R × T
ς = m / V
relate the moles (n) to the mass (m) via the molecular weight (M)
n = m / M m = n × M
V = n × R × T / p
ς = p × M / (R × T)
5. DALTON’S LAW
Dalton
(1801)
pure gases
gas mixtures
(atmospheres)
DALTON’S LAW
the total pressure of a gas mixture, p, is the sum of the
pressures of the individual gases (partial pressures) at a
constant temperature and volume
p = pA + pB + pC + ….
pA × V = nA × R × T pA = nA × R × T / V
pB × V = nB × R × T
p × V = n × R × T
pB = nB × R × T / V
p = pA + pB
p = (nA + nB) × R × T / V
p × V = n × R × T
pA = nA × R × T / V
p × V = (nA + nB) × R × T
pA / p = nA /(nA + nB) = xA
mole fraction
x < 1
pA = xA × p
A gas mixture contains 4.46 moles of neon, 0.74 moles of Ar, and 2.15 moles of xenon. Calculate
the partial pressure of each gas if the total pressure is 2.0 atm.
2 KClO3 → 2 KCl + 3 O2
SUMMARY
p × V = n × R × T
1. ideal gas equation
R = 8.314 J / mol / K
Vm = 22.4 l
2. molar volume
ς = p × M / (R × T)
3. Density of gases
4. Dalton’s Law
p = Σ pii=1
n
Homework
Chapter 5, p. 166-179problems