Modern vacuum pumps make it easy to attain pressures of the order of 10${^-}{^1}{^3}$ atm in the laboratory. Consider a volume of air and treat the air as an ideal gas. (a) At a pressure of 9.00$\times$ 10${^-}{^1}{^4}$ atm and an ordinary temperature of 300.0 K, how many molecules are present in a volume of 1.00 cm$^3$? (b) How many molecules would be present at the same temperature but at 1.00 atm instead?
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Step 1
00 \times 10^{-14}\) atm Volume, \(V = 1.00\) cm\(^3\) = \(1.00 \times 10^{-6}\) m\(^3\) (converted from cm\(^3\) to m\(^3\)) Universal gas constant, \(R = 8.314\) J/(mol·K) Temperature, \(T = 300.0\) K Show more…
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Adi S.
Modern vacuum pumps make it easy to attain pressures of the order of $10^{-13}$ atm in the laboratory. Consider a volume of air and treat the air as an ideal gas. (a) At a pressure of $9.05 \times 10^{-14}$ atm and an ordinary temperature of $295.0 \mathrm{~K}$, how many molecules are present in a volume of $1.05 \mathrm{~cm}^{3} ?$ (b) How many molecules would be present at the same temperature but at 1.10 atm instead?
$\bullet$ Modern vacuum pumps make it easy to attain pressures on the order of $10^{-13}$ atm in the laboratory. At a pressure of $9.00 \times 10^{-14}$ atm and an ordinary temperature of $300 \mathrm{K},$ how many molecules are present in 1.00 $\mathrm{cm}^{3}$ of gas?
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