Question
(a) How many moles per cubic meter of an ideal gas are there at a pressure of $1.00 \times 10^{14} \mathrm{N} / \mathrm{m}^{2}$ and at $0^{\circ} \mathrm{C}$ ? (b) What is unreasonable about this result? (c) Which premise or assumption is responsible?
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Here, $P$ is the pressure, $V$ is the volume, $n$ is the number of moles, $R$ is the gas constant, and $T$ is the temperature. Show more…
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Unreasonable Results (a) How many moles per cubic meter of an ideal gas are there at a pressure of $1.00 \times 10^{14} \mathrm{N} / \mathrm{m}^{2}$ and at $0^{\circ} \mathrm{C} ?(\mathrm{b})$ what s unreasonable about this result? (c) Which premise or assumption is responsible?
(a) Find the number of moles in one cubic meter of an ideal gas at $20.0^{\circ} \mathrm{C}$ and atmospheric pressure. (b) For air, Avogadro's number of molecules has mass 28.9 $\mathrm{g}$ . Calculate the mass of one cubic meter of air. (c) State how this result compares with the tabulated density of air at $20.0^{\circ} \mathrm{C}$ .
(a) Find the number of moles in one cubic meter of an ideal gas at $20.0^{\circ} \mathrm{C}$ and atmospheric pressure. (b) For air, Avogadro's number of molecules has mass 28.9 $\mathrm{g}$ . Calculate the mass of one cubic meter of air. State how the result compares with the tabulated density of air.
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