O2 Water

Question: Fish generally need an O2 concentration in water of at least 4 mg/L for survival. What partial pressure of oxy? What partial pressure of oxygen above the water (in atmospheres at 0 C ) is needed to obtain this concentration? The solubility of O2 in water at 0 C and 1 atm partial pressure is . 2.21 x 10^-3 mol/L

Answer: 2e-3 mol dissolved O2/ L = 1 atm O2 gas (we'll use this as a conversion factor in a moment) (4 mg / L) / (16 g / mol) = 0.25 mmol O2 / L (0.25 mmol O2 / L) (1 atm O2 gas / 2e-3 mol O2/ L) = 0.125 atm O2 gas m

Question: how to remove the water of compressed N2 and O2 thoroughly? Absolute dryness is very important for my experiment, so the N2 and O2 from cylinder must be gotten rid of water thoroughly, the flow tate of them are about 0.8L/h, if someone know the method, please tell me, I will be very appriciated

Answer: we used solid, dry CaCl2 in the lab, with a bit of CoCl2 as an indicator, although CaSO4 and CaO would work too. the reaction of CaO is exothermic, so it wouldn't be good if you have too much water.

Question: how many moles oh H2 in excess when 2 moles of H2 react with 1 mole of O2 to form water? how many moles oh H2 in excess when 2 moles of H2 react with 1 mole of O2 to form water?

Answer: 2 H2 + O2 = 2 H2O H2 is not in excess

Question: how many moles of H2 are needed to convert 5.0 moles of O2 to water? also, how many moles of H2 are needed to convert 5.0 moles of O2 to hydrogen peroxide, H2O2? can somebody please explain to me how these mole equations work? cheers.

Answer: Write out the chemical equations. 2H2 + O2 -> 2H2O H2 + O2 -> H2O2 For water, you need twice as many moles of hydrogen as oxygen, so for 5 moles O2 you need 10 moles H2. For hydrogen peroxide, you need equal amounts, so 5 moles of hydrogen for 5 moles of oxygen.

Question: When H2 and O2 react and water vapor is produced, what type of reaction is that? Can you please tell me how you found that out? Thanks a lot!

Answer: There a few different types of reactions: Combination - where two or more atoms are combined to form a compound. Decomposition - where a compound is decomposed into smaller parts. Single-replacement - usually a compound and an atom are reacted, and the atom basically trades places with another atom in the compound. Double-replacement - usually where two compounds are reacted and the cation + anions of the compounds trade places. Combustion - where a fuel and O2 react to produce CO2 and water vapor. The reaction of 2H2 + O2 -> 2H2O + heat is technically a combustion reaction used to power rocket engines, but since CO2 is not produced for the purposes of a general chemistry course I'd go with Combination.

Question: cleaning my 6 months baby ear using water and vinegar or water and O2 solution? the doctor said i should clean my baby's ear with warm water and oxygen or warm water and vinegar but she really didnt explain how to do the whole thing ! could any 1 please help and will it hurt my baby ? and how EXACTLY to do it ? and wat is best and less irritating to use te vinegar or O2 solution . thank you in advance

Answer: I have not ever heard of such a thing for babies. Adults, yes, children (at least babies-no). I sometimes wash my ears out with warm water and hydrogen peroxide. A tiny bit. I don't know about doing your baby's ears. Just a tissue with your pinky finger to clean the ears I would think should be okay. I have heard that sometimes water in the ear can cause ear infections. I'm concerned because you aren't doing it to your ears, you are doing it to your baby's ears, and you can only see, not feel what is going on. Take care.

Question: can a person really drink the substance of O2 just lsike water ? or is it going to effect my stomach ?

Answer: By O2, I'm usuming you mean oxygen, this would obviously be impossible as O2 is a gass and water is a liquid. You could, of course, simply gulp down air - this wouldn't effect your stomach if you didn't do it endlessy, but may cause flatulence. If, however you mean "Liquid Oxygen", I'm afraid that would be impossible to drink, as Liquid Oxygen must be kept at extremely low temperature, nearly absolute zero. The process of bringing it to your mouth would vaporize it. Also, drinking anything at this low temperature would freeze your mouth, and do damage. Remember that air isn't just O2, but a mixture of Oxygen, Nitrogen and Carbon Dioxide. Breathing or drinking pure oxygen is vast ammount can kill you. Hope that helps!

Question: How much water does a H2/O2 fuel cell produce? How would this be determined? What variables affect the volume of water produced per watt/kilowatt? If a cell is loaded heavily, does it produce more/less/same amount of water per watt than if it is lightly loaded?

Answer: 1. The PEM fuel cell works by migrating the protons through a membrane. So, for each H2O molecule, you get 2 electrons. Use molar weights to determine amount of water. Power = E * I, where I is coulomb per second. Look up number of electrons per coul to calculate. 2. The efficiency. This is a function of voltage drops and unreacted fuel, see article. 3. Less.

Question: The rate equation for the synthesis of water 2H2+O2--> 2H2O is Rate = k[H2][O2] What is the overall orde? The rate equation for the synthesis of water 2H2 + O2 --> 2H2O is Rate = k[H2][O2] What is the overall order of this reaction? 0 1 2 3 Thank so much!!

Answer: 3rd order because the coefficient of H2 is 2, so you raise it to the 2nd power in the rate equation.

Question: How many L of O2 are released from the decomp of 3.6 L of hydrogen perox. gas to produce water vapor + oxygen? Volume - Volume How many liters of O2 are released from the decomposition of 3.6 L of hydrogen peroxide gas to produce water vapor and oxygen? Please show the process.

Answer: 2 H2O2 --> 2 H2O & O2 the identical ratio of 2 moles H2O2 produces 2 moles of H2O tells us that those two gases also ratio in volume 1 to 1 so 3.6 Litresf H2O2 produces gas your answer: 3.6 litres of H2O gas

Question: How many grams of water can be produced by the reaction of 2.40 mol C2H2 with 7.40 mole O2? the heat from an acetylene torch is produced by burning acetylene (C2H2) in oxygen. 2C2H2(g) + 5O2(g)--->4CO2(g)+2H2O(g) How many grams of water can be produced by the reaction of 2.40 mol C2H2 with 7.40 mole O2?

Answer: This is a limiting reactants problem. This would be quite hard to explain in this box, so basically you end up finding that you use all of the C2H2 up before the O2, so the C2H2 is your limiting reactant, and you use 2.40 moles of it. the coefficients of the C2H2 and the H2O are the same, 2. So the There are the same number of moles of H20 created as there are C2H2 used up. 2.40 moles of H2O are created, and when you convert this to grams you get 43.2 g (to the correct number of sig figs)

Question: How much O2 does a regular fish tank water plant produce compared to oxygen consumption by gold fish? I basically just want to know how many small water plants I should put in my fish bowl to provide a decent amount of oxygen for my fish to live on, rather than putting in an air pump. Plants just seem more natural, and it would be kinda cool having a mini ecosystem in my fishbowl. lol.

Answer: A bowl huh? I don't know how many plants. Just put in whatever will fit. Make it look good. Everything should be just fine then.

Question: if 10g of H2 reacted with 160g of O2 which will be the limiting reagent & how many grams of water is produced? for the following reaction 2 H2 + O2----> 2 H2O if 10g of H2 is reacted with 160g of O2 which is limiting reagent and how many grams of water will be produced?

Answer: in order to find the limiting reactant, calculate the number of moles present of each reactant and then divide by the corresponding coefficient in the balanced equation. the smaller result is for the limiting reactant moles O2 = 160g / 32.0g/mol = 5.0 moles divided by the coefficient: 5.0 moles moles H2 = 10g/2.0 g/mol = 5.0moles divided by the coefficient: 5.0 moles/2 = 2.5 moles the limiting reactant is H2 according to the balanced equation, moles H2O produced equals the moles H2 reacted. i.e. 5 moles mass water = 5moles * 18g/mol = 90g

Question: How does H2O separate in to H2 and O2 in the process of electrolysis of water? Don't give me wikipedia as a source, it's too complicated.

Answer: when electricity is passed through water, H+ & O- are actually obtained.so H+ goes to cathode & O- goes to anode (opposite charges attract each other) O- gives electron to anode(to become O) which is transferred to cathode.This electron is taken by H+ (which is already present in cathode) to become H. Then O combines with another O to become O2 H combines with another to become H2 H2 & O2 are obtained separately in 2 different test tubes(placed over cathode & anode respectively).

Question: Fish generally need an O2 concentration in water of at least 4 mg/L for survival. What partial pressure? 2.Fish generally need an O2 concentration in water of at least 4 mg/L for survival. What partial pressure of oxygen above the water (in atmospheres at 0°C) is needed to obtain this concentration? The solubility of O2 in water at 0 °C and 1 atm partial pressure is 2.21 x 10-3 mol/L.

Answer: First change 4 mg/L to mol/L, by dividing 0.004 g by the weight of 1 mol O2. Call this FishMol. Henry's Law says solubility of a gas in a liquid is directly proportional to partial pressure of the gas over the liquid, so divide FishMol by the solubility (2.2*10^-3 mol/L-Atm) and you get the required O2 partial pressure in Atm. The answer could be 0.05656 but I could be lying or wrong.

Question: Does boiling a pot of water release oxygen from it? If so, is it breaking apart H2O or releasing disolved O2? My roomate and I are debating wheather oxygen is released from water when boiled. I say that boiling would not break any oxygen from the H2O molecules. But, I realized maybe it would release the oxygen dissolved in the water, like what fish breath. What is the answer?

Answer: you are both correct - the boiling process does not chemically change water into the elements hydrogen and oxygen, but the higher temperature will drive out any dissolved oxygen that was in the water (gases are less soluble in liquids at higher temperatures than lower temperatures)