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17

There's a NASA report that looks into this: "ON THE SOLUBILITIES AND RATES OF SOLUTION OF GASES IN LIQUID METHANE", Hibbard and Evans, 1968 and concludes that such mixtures are possible. Starting on page 8: Figure 5(a) presents the curves for oxygen, argon, carbon monoxide, and nitrogen. Also shown are the two experimental values for nitrogen. ...


10

Caesium salts are unapologetically ionic, and they typically have quite high mass solubilities in many solvents, including water. Assuming organic ions are allowed, caesium acetate ($\ce{H3CCO2^-Cs+}$) in particular has a remarkably high solubility of 9451 g/kg water at −2.5 °C, increasing to 13 455 g/L water at 88.5 °C. Caesium formate ($\ce{HCO2^-Cs+}$) ...


9

The following data is compiled from [1, pp. 4-44, 5-167]: Table 1. Selected solubility values of the inorganic compounds with significant ionic character at $25~\mathrm{^\circ C}$. $$ \begin{array}{lc} \hline \text{Formula} & \text{Solubility in water}/\pu{g L-1}\\ \hline \ce{CsF} & 5730\\ \ce{SbF3} & 4920\\ \ce{LiClO3} & 4587\\ \ce{Pb(ClO4)...


8

To add to the Bob's excellent answer (and expand a bit on my comment there), I've found two other potentially interesting papers to peruse. The first is R.J. Hodges and R.J. Burch, Cryogenics 7 112-113 (1967), titled "The equilibrium distribution of methane between the liquid and vapour phases of oxygen". They note a "very high solubility of methane in ...


8

There is not going to be a single definitive answer, primarily because of a wide gray zone surrounding the domain of ionic compounds. Besides, as Nikolau noted, the question is ambiguous. If you want mass concentration, then look at $\ce{InI3}$ which claims a whopping $13100~\mathrm{g/L}$. Pity that it is probably ionic in name only, judging by the ...


4

We can do better than that. Ammonium nitrate = 1500 g/L at 20°C.


3

Technically, a smooth or molten, unoxidized metal surface (regardless of chemistry) makes a good candidate. This thesis from Auburn University reports the emissivities of both oxidized and unoxidized metals at temperatures typically encountered in industrial processes; note the low values for all the unoxidized metals studied in the IR range where most ...


3

The nearest to an ideal fluid is a hard sphere fluid, but this is removed from the ideal gas or even solution concept of ideality in a critical way. Ideal (also called perfect) gases are ideal because they lack intermolecular interactions. A statistical description that ignores the intermolecular potential suffices to describe an ideal gas. A first ...


2

I will first enumerate the four points that need to be addressed. The vapor and liquid phases have the same composition in an azeotrope. The azeotrope boils at a constant temperature. The composition of the azeotrope remains fixed while boiling. The azeotropic mixture cannot be separated by fractional distillation. I will assume the definition of an ...


2

Definitions and facts Boiling point - when the vapour pressure of the solution is equal to the atompheric pressure, then it is said to be boiling. Vapour pressure - sometimes molecules escape the solution to convert into the gas phase, also molecules in the gas phase combine to turn back into liquid phase. Hence there exists a equilibrium between gas phase ...


2

There are several redox reactions can be taken place when you add household beach on elemental mercury metal. However, this question is more like a homework question. Thus, I give you insight to the answer and you may read a bit and find out what's happening. This reaction is studies and results have been published (Reference 1), the abstract of which states ...


1

Is it predefined/can be computed based on the substance or is it irrelevant? The state symbols, l, s, g, (aq), as they are called are nothing but qualitative descriptors. They have nothing to do with concentrations. It is a good point when do we distinguish (l) and (aq)? You have already answered it. When a given component in the equation is a pure liquid ...


1

I would take a look at this thread A boiling point question. A crude answer to this is that it takes work for a molecule to "squeeze" or "jump" from one phase into another. Liquids are tightly packed but vapor is quickly moving. A possible analogy is that moving into the liquid is like squeezing a marble into a full jar of marbles whereas moving into the ...


1

Wikipedia disagrees with your figures. They give a melting point only for the pentahydrate (18°C, at which point this forms not pure sodium hypochlirite but a solution of one mole sodium hypochlirite to five moles water). The only reported phase transition for the neat compound is a "boiling point" of 101°C which is actually a decomposition point. So I ...


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