410.8g + 3286.4g = 3697.2g (only 2.8g off from our assumed mass for volume, and an overall error of just 0.07% for rounding/approximation errors). You can see that although the volumetric ratio of the reactants is 2:1 for hydrogen:oxygen, the mass ratio is 1:8! We can check our calculations by adding up the calculated reactant masses and comparing them to the final product mass. This demonstrates the utility and necessity of using molar quantities for chemical reactions. The volume of oxygen required is 102.7 moles * 22.4L/mol = 2300L. To convert: To: Do This: Liters Gallons Divide By 3.8 Quarts Gallons Divide By 4 Gallons Liters Multiply By 3. Divide 359 by the molecular weight of the gas. The volume of hydrogen required is 205.4 moles * 22.4L/mol = 4601L. Oxygen O2 11.1 105.8 Perfluoropropane (see Freon 218) C3F8 1.9. The volumes required (uncompressed) can be derived from the approximation of 22.4L/mol for ideal gases. The mass of oxygen required is 102.7 moles * 32g/mol = 3286.4 grams. The mass of hydrogen required is 205.4 moles * 2g/mol = 410.8 grams. The weight of a cryogenic liquid in the tank must be determined by weighing. ![]() If you want to convert those values into either mass or volumes (at standard temperature and pressure) we can apply the appropriate conversion factors. oxygen, cryogenic liquid or any flammable cryogenic liquid. Oxygen at 230 psi has a product weight of 379 pounds. of a modern internal combustion engine car with equivalent gas in the tank, which works out to a gasoline-per-gallon equivalent between 5 and 6. This tells us that to end up with 205.4 Moles of water, we must combine 205.4 moles of hydrogen with 102.7 moles of oxygen because the equation ratios are 2:1:2 respectively. Compare this weight to the regis- tered tare weight on the data plate. Where quantities are indicated in pounds and when the weight per gallon of the liquid is not provided to the AHJ, a conversion factor of 10 lb/gal (1.2 kg/L). The chemical equation for the combination of hydrogen and oxygen defines the ratios at which molar quantities react: Now we use the molar definition to find that 3700g of water (in any form) will consist of 3700g/18.01 g/mol = 205.4 Moles of water. You can estimate the density of a substance by weighing a known volume of it. Do not permit liquid oxygen or oxygen-enriched air to come in contact with organic materials or flammable or combustible substances of any kind. Working backwards from the stipulated product quantity we have water mass at 1 gram/milliliter, resulting in a final mass of 3700g of water. 1 cubic foot (ft3) of water is equal to 62.4 lbs AND 7.48 gallons. Sizes range from 500 to 420,000 gallons (1,893 1,589,873 Liters). If you'll allow me to use metric units instead of English ones (although the UK has gone metric for a long time itself) I will use the conversion of 1 gallon to 3.7 liters, or 3700mL. That's a very good question to demonstrate the use of molar quantities in converting from one state (gaseous reactants) to another (liquid product).
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