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By accessing this web page or using these results in any manner whatsoever, you agree to be bound by the foregoing restrictions.https://chemistry.stackexchange.com/questions/65979/what-is-the-difference-between-o-o2So, to reiterate, the difference between oxygen $\left (\ce O\right)$ and oxygen $\left (\ce {O2}\right)$ is that the former is an oxygen atom while the latter consists of two $\ce O$ atoms bound together, forming a molecule also called oxygen.Wed, 22 Apr 2026 23:37:00 GMThttps://chemistry.stackexchange.com/questions/9552/ch4-o2-co2-2h2-whats-wrong-with-itThere's nothing wrong. It's incomplete combustion. It is one of a number of oxidizing reactions that can and will be occurring if you are burning this hydrocarbon in an oxygen-restricted environment. But the dominant reaction will be the one where the lowest energy state is reached. So you will likely wind up with one CO molecule, one water molecule and one hydrogen molecule instead.Sun, 19 Apr 2026 13:39:00 GMThttps://chemistry.stackexchange.com/questions/15126/enthalpy-of-the-reaction-between-hydrogen-and-oxygenIn this case, the enthalpy of $484\ \mathrm {kJ}$ is released when $2\ \mathrm {mol}$ of hydrogen gas react with $1\ \mathrm {mol}$ of oxygen gas to form $2\ \mathrm {mol}$ of gaseous water: $$\ce {2H2 (g) + O2 (g) -> 2H2O (g)}\qquad\Delta H^\circ = -484\ \mathrm {kJ}$$ (By way of comparison, the corresponding value for liquid water is about ...Thu, 23 Apr 2026 19:25:00 GMThttps://chemistry.stackexchange.com/questions/169849/what-form-of-energy-is-produced-by-2h2-o2-2h2o-reaction0 Thermal energy is released from the reaction $\ce {2H2 + O2 -> 2H2O}$. Before the reaction takes place the system of $\ce {H2}$ and $\ce {O2}$ molecules are in a metastable state: Given enough energy > activation energy the system gains enough energy to overcome the potential barrier and falls into a state of lower energy than the initial state.Sat, 11 Apr 2026 08:12:00 GMThttps://chemistry.stackexchange.com/questions/915/how-can-carbon-dioxide-be-converted-into-carbon-and-oxygen$\ce {CO2}$ into $\ce {CO + O2}$ is easier, but you need a catalyst and about $\pu {1500 °C}$ as reported by Richard Van Noorden’ article “ Recycling carbon dioxide into petrol ” about the Sandia reactor, 2008-01-03 (WBM link).Fri, 24 Apr 2026 06:10:00 GMThttps://chemistry.stackexchange.com/questions/14647/if-co2-is-nonpolar-how-come-much-more-dissolves-in-water-than-o2Both of these factors will stabilize a $\ce {CO2}$ molecule more than an $\ce {O2}$ molecule in water; stabilization translates into greater solubility.Thu, 23 Apr 2026 23:50:00 GMThttps://chemistry.stackexchange.com/questions/73565/why-are-some-molecules-unable-to-absorb-infrared-radiationAll homo-nuclear diatomics, $\ce {N2}$, $\ce {O2}$ for example, are transparent to IR radiation and this is of prime importance in global warming, since if these molecules obtain energy, say by collision with water or carbon dioxide that has been excited by IR radiation, they cannot radiate the energy away and so must heat the atmosphere by ...Wed, 22 Apr 2026 20:52:00 GMThttps://chemistry.stackexchange.com/questions/104791/why-do-we-call-o2-oxygenLikewise $\ce {O2}$ is as much oxygen as atomic oxygen is. The only complication is that what we habitually think of as oxygen is oxygen as a gas comprised of $\ce {O2}$ molecules. Like Humpty Dumpty in Alice in Wonderland, "a word means what [we] choose it to mean" and often we have to add modifiers or alternate terms to avoid ambiguity.Mon, 20 Apr 2026 02:32:00 GMThttps://chemistry.stackexchange.com/questions/8364/determining-standard-gibbs-free-energy-for-waterLet's look at the reaction of the formation of water: $\ce {2H2 (g) + O2 (g) -> 2H2O (l) }$ The Gibb's Free Energy relates the spontaneity of various reactions by looking at the change in enthalpy, temperature, and entropy. We can relate those by: $$ \Delta G^\circ = \Delta H^\circ - T\Delta S^\circ$$ If we look at our reaction, it's clear that this is an exothermic reaction. Bonds are being ...Fri, 24 Apr 2026 15:21:00 GMThttps://chemistry.stackexchange.com/questions/164207/why-is-the-boiling-point-of-fluorine-lower-than-that-of-oxygenNitric oxide combines a weak dipole with the dimerization capability between molecules with an unpaired electron, forming a dimer. The tendency of nitric oxide to dimerize, though weak, is stronger than that in $\ce {O2}$, so this interaction produces a larger effect on boiling point with the nitrogen oxide.Thu, 23 Apr 2026 04:38:00 GMT