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Barium (Ba) has an At. No. of 56, and an At. Wt. of 137.36.
(7.8 gm moles) X (137.36 gm/gm mole) = 1071.408 gm.
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∙ 11y ago
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∙ 11y ago411.98 grams
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How many moles contained in 14.2g of barium sulfate?
The molar mass of barium sulfate, BaSO4 is 233.4 Amount of BaSO4 = mass of sample / molar mass = 14.2/233.4 = 0.0608mol 0.0608 moles of BaSO4 are conained in a 14.2g pure sample.
How many moles are in 317.0 g of BaOH2?
Molar mass of barium hydroxide, Ba(OH)2 = 171.3Amount of barium hydroxide = mass of sample / molar mass = 317.0/171.3 = 1.85mol
What is the mass of 3 moles in ammonia?
One mole approximately weighs 17g.So 3 moles have a mass of 51g.
What is the mass of 4.80 mol of barium hydride?
4.32 moles Barium (6.022 X 10^23/1 mole Ba) = 2.60 X 10^24 atoms
Mass of 3 moles of ammonia?
Molar mass of ammonia = (14.01 + 3.03) (Molar mass of nitrogen + 3 times molar mass of hydrogen, as chemical formula of ammonia is NH3). Molar mass= 17.04 Molar mass x moles = mass 17.04 x 3 = 51.12 Mass of 3 moles of ammonia is 51.12g.
How many moles of barium are present in a sample having a mass of 22.3 grams?
# of moles = grams of substance / molar mass of substance molar mass of Barium =137.33 grams/mole #moles of Barium = 22.3 grams/ 137.33 grams/mole = 0.162382582 moles
How many moles contained in 14.2g of barium sulfate?
The molar mass of barium sulfate, BaSO4 is 233.4 Amount of BaSO4 = mass of sample / molar mass = 14.2/233.4 = 0.0608mol 0.0608 moles of BaSO4 are conained in a 14.2g pure sample.
How many moles are in 317.0 g of BaOH2?
Molar mass of barium hydroxide, Ba(OH)2 = 171.3Amount of barium hydroxide = mass of sample / molar mass = 317.0/171.3 = 1.85mol
What is the mass of one mole of barium nitrate?
First, we need to find the formula for barium nitrate. Barium's charge is 2+, and nitrate is a 1-. If you criss-cross charges, the resulting formula is Ba(NO3)2. Now that we have the formula, we need to find the atomic mass. Barium has an atomic mass of 137. Nitrate is composed of nitrogen (14.01g) and oxygen (16.00*3 = 48). The atomic mass of nitrate is 62.01. Since there are two NO3 molecules, we multiply by 2 to get 124.02. Finally, we add the barium for a grand total of 261.02. Finally, we set-up our conversion ratios: 432 g Ba(NO3)2/1 * 1 mol/261.02g = 1.66 mols
How many moles of barium sulfate are produced from 0.100 mole of barium chloride?
Since both barium chloride and barium sulfate contain one mole of barium atoms pert mole of compound, the moles of barium sulfate will be the same, 0.100, when barium has the limiting concentration in the production of the sulfate.
What is the mass of 3 moles in ammonia?
One mole approximately weighs 17g.So 3 moles have a mass of 51g.
Barium hydroxide contained 2.74g in 100cm of water titration of 20cm required 18.7cm of a hydrochloric acid solution for complete neutralization what is the molarity of the barium hydroxide?
Barium Hydroxide: Mass: 2.74g. Mr = 171. Moles = Mass (g)/Mr Therefore - 2.74/ 171 = 0.01602339181mols.
Mass of 3 moles of ammonia would be?
The molar mass of ammonia is about 17 grams, so that 3 moles would have a mass of 51 grams.
Mass of 3 moles of ammonia?
Molar mass of ammonia = (14.01 + 3.03) (Molar mass of nitrogen + 3 times molar mass of hydrogen, as chemical formula of ammonia is NH3). Molar mass= 17.04 Molar mass x moles = mass 17.04 x 3 = 51.12 Mass of 3 moles of ammonia is 51.12g.
What is the mass of 4.80 mol of barium hydride?
4.32 moles Barium (6.022 X 10^23/1 mole Ba) = 2.60 X 10^24 atoms
What is the molarity of 2 moles of compound dissolved in r L of water?
Need to know the mass of BaCl2 in order to calculate molarity.
What is the molar mass equivalent to 50 mol. of barium nitrate?
The formula of (unhydrated) barium nitrate is Ba(NO3)2. This means, among other things, that each mole contain one mole of barium atoms, two moles of nitrogen atoms, and six moles of oxygen atoms. Thus, the molar mass of this compound is 137.327 + 2(14.007) + 6(15.999) = 261 grams, to three significant digits. 50 moles will then be fifty times this or 1.3 kilograms, to the justified number of significant digits.
