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The pressure required to reach this point is called the critical pressure which, for hydrogen, is $\pu{1.239 MPa} = \pu{179.7 psi}$. Hence, while you can't change hydrogen into a liquid at room temperature, you can change it into a (supercritical) fluid. Incidentally, there are two established storage technologies for pure hydrogen in vehicles.
Well, first of all depends on what temperature you are considering. But let’s take room temperature (20 degrees). In Water, the oxygen atom is highly electronegative and can polarize (partially) the hydrogen atoms, thus hydrogen-hydrogen bonds between the H2O molecules can be formed creating a very high boiling point.
Therefore, the reaction must be specified for which this quantity applies. In this case, the enthalpy of 484 kJ 484 k J is released when 2 mol 2 m o l of hydrogen gas react with 1 mol 1 m o l of oxygen gas to form 2 mol 2 m o l of gaseous water: 2HX2(g) +OX2(g) 2HX2O(g) ΔH∘ = −484 kJ 2 H X 2 (g) + O X 2 (g) 2 H X 2 O (g) Δ H ∘ = − 484 ...
Yes, if the HX2(g) H X 2 (g) concentration in oxygen or air is greater than about 4% not only will it burn, but most likely explode. You should avoid all heat sources when dealing with it, including direct sunlight. Just so you know, hydrogen safety datasheets include words such as "extremely flammable" and "DANGER" in red capital letters.
Water has stronger hydrogen bonds than ice does. Liquid water is denser than ice. Since water and ice are both made of H2O molecules, the fact that water is denser means the H2O molecules are closer together in water than they are in ice. This means the intermolecular forces attracting one H2O molecule to another must be stronger in water than ...
The boiling point of hydrogen is $-252.87~^{\circ}\rm C$ or $20.28\rm\,K$, which is the least boiling point so you can expect that all other elements would liquidify or solidify at or below this temperature. But the concept of phases is much more complicated than that.
I'm sure most of us have heard that saturated fats are solid at room temperature, and unsaturated fats are liquid at room temperature. I'm wondering how this relates to their chemical structure -- saturated fats contain only single bonds between carbons, yet to qualify as an unsaturated fat a C=C double bond must exist.
It is a gas at room temperature with a boiling point ϑb = −23.8 ∘C ϑ b = − 23.8 ∘ C. Chloroform, which is indeed a liquid at room temperature (ϑb = 61.2 ∘C ϑ b = 61.2 ∘ C) is CHClX3 C H C l X 3 or trichloromethane. You need to substitute three hydrogens with chlorine atoms to create chloroform. Share. Cite.
1,151 6 15 23. Add a comment. Yes. Temperature disrupts bond of all kinds. Heat up a protein hot enough and you can even disrupt its primary structure - the linear sequence of amino acids, and amino acids are held together through covalent bonds. This is why prion contaminated organisms and instruments must be heated to extremely, extremely ...
2. The commonly cited reason is inter-molecular hydrogen bonding. But won't the hydrogen bonding in phenol be weaker than that of most alcohols because of resonance-effect? And yet, alcohols with stronger hydrogen bonding (such as ethanol, propanol, etc.) aren't solids at room temperature. Also, if the reason behind its state is it's molecular ...