what happens when we change the quantity of gas? when using the combined gas law, n is constant. law...
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What happens when we change the quantity of gas? When using the combined gas law, n is constant.
Law of Combining Volumes
See Fig. 1 on p. 576
Which test tube contains H2(g)?
2 H2O(g) 2 H2(g) + O2 (g)
Gay-Lussac’s Law of Combining Volumes: when gases react, the volumes of the reactants and products, measured at equal temperatures and pressures, are always in whole number ratios
(whole number ratios are the stoichiometric coefficients)
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How can 2 samples of gas that contain particles of different mass have equal pressures at the same T?
Avogadro’s Hypothesis: equal volumes of all ideal gases at the same T and P contain the same number of molecules Fig 4 p. 578
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Molar Volume At STP, 1 mole of an ideal gas will have a volume of ______.
At SATP, 1 mole of an ideal gas will have a volume of 24.8 L.
Then how do gases differ from one another??? mass (due to different molar masses) density
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Ideal Gas LawR= universal gas constant
Derive R @ STP…
R= 8.314 kPa L/mol K
R= 0.082058 atm L/ mol K
R= 62.37 mmHg L/ mol K
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Dalton’s Law of Partial Pressures
Imagine mixing 3 different gases each having a different pressure…
What would the final pressure be?
Dalton’s Law of Partial Pressures: the total pressure of a mixture of gases is the sum of the pressures of each of the individual gases
Ex. What is the pressure of O2 in the atmosphere?
Ptotal= P1 + P2 + P3 + … +Pn
PracticePg. 594 #1-4Pg. 596 #1-3