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2 Chemistry questions help please?
1. A hot-air balloon rises. Explain why using your knowledge of gases and gas laws.
2. Four moles of He(g) and four moles of Ar(g) are placed in a glass vessel at room temperature. The partial pressures of the gasses initially total 12.0 atm. Then the vessel springs a pinhole-sized leak, and 1.00 mole of He(g) effuses. What are the partial pressures of each gas remaining in the glass vessel now?
1. The hot air in the hot air balloon is the same pressure and higher temperature than the surrounding air. As a result, the air in the balloon is less dense
2. Graham's Law of Effusion is
Rate Ar = Rate He * sqrt(MW He / MW Ar)
Since moles is proportional to rate
Moles Ar = Moles He * sqrt(MW He / MW Ar)
= 1.00mol * sqrt(4.003 / 39.95)
Moles Ar = 0.317mol Ar
Calculate the remaining moles of Ar
Remaining moles Ar = 4.00mol Ar - 0.317mol Ar
Remaining moles Ar = 3.68 mol Ar
The ideal gas law is
PV = nRT
If the volume and temperature are constant
P1 / n1 = P2 / n2
P2 = P1 * n2 / n1
= 12.0atm Ar * (3.68mol Ar / 4.00mol Ar)
P2 Ar = 11.1atm Ar
For helium
Remaining moles He = 4.00mol He - 1.00mol He
Remaining moles He = 3.00mol He
P2 = P1 * n2 / n1
= 12.0atm He * (3.00mol He / 4.00mol He)
P2 He = 9.0atm He
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