Calculate the degrees of freedom and number of components for a system of sodium chloride solution containing undissolved salt in equilibrium with water vapour
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Calculate the degrees of freedom and number of components for a system of sodium chloride solution containing undissolved salt in equilibrium with water vapour
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- 7.5. For this chemical equilibrium in an enclosed system, how many degrees of freedom are there?How many phases and component are present in (a) homogeneous system (b) an aqueous solution of salt (c) toluene in equilibrium with its vapourIdentify the number of degrees of freedom and potential intensive variables for a mixture of benzene and toluene in equilibrium with the vapor phase.
- When a two-component system has two phases, what is the degree of freedom?Using the Gibbs phase rule determine the number of components, number of phases and hence the number of degree of freedom using the Gibbs phase rule for each of the following systems: An aqueous solution containing Na+, C?-, K+ and Br- ions.A dilute solution of bromine in carbon tetrachloride behaves as an ideal dilute solution. The vapour pressure of pure CCl4 is 33.85 Torr at 298 K. The Henry’s law constant when the concentration of Br2 is expressed as a mole fraction is 122.36 Torr. Calculate the vapour pressure of each component, the total pressure, and the composition of the vapour phase when the mole fraction of Br2 is 0.050, on the assumption that the conditions of the ideal dilute solution are satisfied at this concentration.
- Determine the number of phases, components, and the variance (degrees of freedom) for the following: (a) A solution made from water, MgCl2 and KBr. (b) A solid mixture containing powdered graphite and powdered diamond. (c) A gaseous mixture containing water and carbon dioxide that was produced from the combustion of a stoichiometric mixture of oxygen and propane gases. Assume the reaction went to completion and there are no residual amounts of propane nor oxygen present. (d) A system containing PCl5(g), PCl3(g) and Cl2(g) in equilibrium. (e) Oxygen gas and hydrogen gas in equilibrium with liquid water.Establish the phase equilibrium for nonreacting systems in terms of the specific Gibbs function of the phases of a pure substanceExplain the concept of partial molar volume, and justify the remark that for a binary solution,the partial molar volume of one component depends on the properties of the othercomponent.
- A saturated solution of copper(ll) sulfate, with excess of the solid, is present in equilibrium with its vapour in a closed vessel. (a) How many phases and components are present? (b) How many degrees of freedom are available, and what are they?The total vapour pressure of an ideal-dilute liquid mixture of acetone and chloroform with a mole fraction of acetone of 0.0500 is 45.08 kPa at 308 K. (a) Use Raou lt's law to determine the partial vapour pressure of acetone for the mixture, given that the vapour pressure of pure acetone is 46.26 kPa at 308 K. (b) Hence calculate the partial vapour pressure of chloroform for the mixture . (c) Determine the Henry's law constant of chloroform at this temperature.(d) The Henry's law constant is lower than the vapour pressureof pure chloroform at 308 K. What does this imply about the nature of the interactions between acetone and chloroform in the liquid mixture?At a temperature of 302.8 K, mixtures of phenol and water exist as two separate phases with mole fractions of phenol of 0.30 and 0.93. Use the lever rule to determine the relative amounts of the two phases for a mixture with an overall mole fraction of phenol of 0.45.