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carbonated water is like regular water only pressurized heavily with carbon dioxide. An airtight sealed and pressurized container is needed to keep the carbon dioxide in the water. Once the container is opened, the sorrounding air and tha low pressure forces the CO2 out of the water causing it to bubble. h2o Hydrogen and oxygen.
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∙ 15y ago
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∙ 14y agoCarbonated water is also known as carbonic acid which has the chemical formula H2CO3.
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∙ 14y agoCarbon dioxide, which reacts with the water in small amounts to form carbonic acid (H2CO3)
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∙ 15y agoH2 .C .O3
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∙ 14y agoH2co3
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How do you find theoretical percent of water?
To find the theoretical percent of water in a compound, you need to determine the molar mass of the compound and the molar mass of water. Then, divide the molar mass of water by the molar mass of the compound and multiply by 100 to get the percentage.
What is a molar mass and what is it used for?
The molar mass is the sum of atomic weight of the atoms contained in a molecule. Example: water, H2O The molar mass is: 2 x 1,008 + 15,999 = 18,015 Molar mass is used in many calculus in chemistry.
How do you calculate the moles of water?
To calculate the moles of water, you can use the formula: moles = mass of water (in grams) / molar mass of water (about 18.015 g/mol). Simply divide the mass of water by its molar mass to find the number of moles.
Calculate The percent Water In CoC2H3O22 x 4H2O?
To calculate the percent water in Co(C2H3O2)2 x 4H2O, first find the molar mass of Co(C2H3O2)2 x 4H2O: 58.93 (Co) + 2*(12.01 (C) + 1.01 (H) + 16.00 (O)) + 4*(18.02 (H2O)). The molar mass is 237.02 g/mol. Next, calculate the molar mass due to water: 4*(18.02) = 72.08 g/mol. The percent water is calculated by (molar mass of water in formula / molar mass of compound) x 100: (72.08 / 237.02) x 100 = 30.42%.
How do you find the molar mass of compounds like water?
The molar mass is the mass of one mole of a substance in g/mol. In order to determine the molar mass, you must know the chemical formula and have access to a periodic table. Let's use water as an example. The chemical formula for water is H2O. To find the molar mass, multiply the atomic weight on the periodic table in grams/mol for each element times the subscript for the element, and add the molar masses. H: 2 x 1.00794g/mol = 2.01588g/mol O: 1 x 15.9994g/mol = 15.9994g/mol ------------------------------------------------ Molar mass = 18.0153g/mol
What the molar mass of water?
The molar mass of water is 18 g/mol.
What is the theoretical percentage of water of hydration in cacl2-2h20?
1. Find the molar mass of the hydrate (Calcium Chloride Dihydrate).Find the molar mass of water and the anhydrate (anhydrate + water = hydrate); add the molar mass values of each to find the molar mass of the hydrate.Molar Mass CaCl2: 110.98g+ Molar Mass H2O: 36.04g*Molar Mass CaCl2 * 2H2O: 147.01gFinding Molar Mass# atoms element A * atomic mass element A = Mass A# atoms element B * atomic mass element B = Mass B... etc.Add up all the mass values and you have the value for molar mass. Do this for both the anhydrate and the water molecules. Add these values together to find the molar mass of the hydrate.Molar Mass Anhydrate + Molar Mass Water Molecules* = Molar Mass Hydrate* Tip: the molar mass of water for all hydrate calculations is 18.02g x number of water molecules. This number may be useful to remember on the day of the test or while doing practice problems.*2. Calculate the percentage of water in hydrate.Divide the molar mass of water by the molar mass of the hydrate, and multiply result by 100%.36.04g147.01g x 100%Percent water in hydrate is 24.52%.
How do you find theoretical percent of water?
To find the theoretical percent of water in a compound, you need to determine the molar mass of the compound and the molar mass of water. Then, divide the molar mass of water by the molar mass of the compound and multiply by 100 to get the percentage.
What is the molar mass of borax after it looses water?
The molar mass of anhydrous borax is 201,22 g.
Molar mass of 158g of ice?
The molar mass of ice is 18.015 g/mol. To find the number of moles in 158g of ice, divide the mass by the molar mass: 158g / 18.015 g/mol = 8.77 moles.
What is a molar mass and what is it used for?
The molar mass is the sum of atomic weight of the atoms contained in a molecule. Example: water, H2O The molar mass is: 2 x 1,008 + 15,999 = 18,015 Molar mass is used in many calculus in chemistry.
A 6.797 g sample of AlCl36H2O is heated until all the water of hydration is removed What will be the mass of the remaining AlCl3?
After heating, the water of hydration will be removed from AlCl3. The molar mass of AlCl3.6H2O is 241.43 g/mol, and the molar mass of water is 18.015 g/mol. By subtracting the molar mass of water from the molar mass of AlCl3.6H2O, we find that the molar mass of AlCl3 is 133.34 g/mol. Therefore, the mass of remaining AlCl3 will be 6.797g / 241.43 g/mol * 133.34 g/mol.
What is the percentage of water in the hydrate CoCl2 and 6H2O Show your work?
To find the percentage of water in CoCl2·6H2O, calculate the molar mass of water (18.015 g/mol) and the molar mass of the whole compound. Molar mass of CoCl2·6H2O = 129.84 g/mol (CoCl2) + 6(18.015 g/mol) = 237.89 g/mol Now, compute the percentage of water: Percentage of water = (6 * 18.015 g/mol) / 237.89 g/mol * 100% ≈ 54.5% Therefore, the hydrate CoCl2·6H2O contains approximately 54.5% water.
Mass of a mole?
The molar mass of an element is its atomic weight in grams. The molar mass of a molecule or compound is the sum of the subscripts times the molar masses in grams. For example, the molar mass of hydrogen, H, is 1.00794g and the molar mass of oxygen, O, is 15.9994g. The molar mass of water, H2O, is (2 x 1.00794g) + (1 x 15.9994g O) = 18.01528g.
What is the percentage of water to the nearest tenth in this compound BaOH2 8H2O?
The compound Ba(OH)2·8H2O has 8 water molecules associated with it. To find the percentage of water in the compound, calculate the molar mass of the water molecules (8H2O) and the molar mass of the entire compound (Ba(OH)2·8H2O). Then divide the molar mass of the water by the molar mass of the entire compound and multiply by 100 to get the percentage of water.
What is the molcular mass of water?
Molar mass of H2O = 18.01528 g/mol
What is the molar mass for anhydrous(without water) barium sulfate?
The molar mass for anhydrous barium sulfate (BaSO4) is 233.43 g/mol
