The solubility of nitrogen gas in rubber at 25^∘ C is 0.00156 kmol / m^3 ·bar. When phase equili

step 1 Question number 118. The density is determined from the molar mass volatility and the pressure o

The solubility of nitrogen gas in rubber at 25^∘ C is...

The solubility of nitrogen gas in rubber at $25^{\circ} \mathrm{C}$ is $0.00156 \mathrm{kmol} / \mathrm{m}^{3} \cdot$ bar. When phase equilibrium is established the density of nitrogen in a rubber piece placed in a nitrogen gas chamber at $300 \mathrm{kPa}$ is $(a) 0.005 \mathrm{kg} / \mathrm{m}^{3}$ $(b) 0.018 \mathrm{kg} / \mathrm{m}^{3}$ $(c) 0.047 \mathrm{kg} / \mathrm{m}^{3}$ $(d) 0.13 \mathrm{kg} / \mathrm{m}^{3}$ $(e) 0.28 \mathrm{kg} / \mathrm{m}^{3}$

The solubility of nitrogen gas in rubber at $25^{\circ} \mathrm{C}$ is $0.00156 \mathrm{kmol} / \mathrm{m}^{3} \cdot$ bar. When phase equilibrium is established the density of nitrogen in a rubber piece placed in a nitrogen gas chamber at $300 \mathrm{kPa}$ is
$(a) 0.005 \mathrm{kg} / \mathrm{m}^{3}$
$(b) 0.018 \mathrm{kg} / \mathrm{m}^{3}$
$(c) 0.047 \mathrm{kg} / \mathrm{m}^{3}$
$(d) 0.13 \mathrm{kg} / \mathrm{m}^{3}$
$(e) 0.28 \mathrm{kg} / \mathrm{m}^{3}$

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Key Concepts

Henry's Law

Henry's Law states that the solubility of a gas in a liquid or solid is directly proportional to the partial pressure of that gas above the medium. This relationship is quantified by the Henry's law constant and is essential in determining how much of a gas will dissolve when equilibrium is established between the gas phase and another phase.

Unit Conversion and Molecular Weight

In many chemical calculations, especially those involving gas solubility, it is necessary to convert between different units of concentration. This often involves converting molar concentrations (such as kmol/m³) to mass concentrations (such as kg/m³) using the molecular weight of the gas. Understanding these conversions is fundamental for accurate quantitative analysis.

Phase Equilibrium

Phase equilibrium involves the state where different phases, such as a gas and a solid, are in balance with each other. At equilibrium, the rate of transfer of species from one phase to another is equal in both directions, implying that the concentration of the species in each phase remains constant over time. This principle is crucial when studying how physical conditions like pressure affect the distribution of a component between phases.

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