What is the mass of c12 h22 o11?
342.3 g/molTable sugar / Molar mass
How do you find the atomic mass of NaOH?
– The atomic weight of the sodium is 23, the atomic weight of the hydrogen is 1, and the atomic weight of the oxygen is 16. – Now we can calculate the molar mass or molecular weight of the sodium hydroxide by using the formula below. Molecular weight of the NaOH= 23 + 1 + (16) = 40.
What is the mass of 2 mole of NaOH?
Solution : 2 mole NaOH 1 mole of NaoH `=40g` of NaOH `=6.023xx10^(22)` molecules 2 mole of NaOH `2xx40g=80g` of NaOH `=2xx6. 023xx10^(23)` molecules.
What is the molecular weight of table sugar sucrose c12 h22 o11 and what is its molar mass in g mol?
342.30 g/mol
Chemical Data of Sucrose
| Chemical Formula of Sucrose | C12H22O11 |
|---|---|
| Molar Mass or Molecular Weight | 342.30 g/mol |
| Density | 1.587 g/cm3 |
| Physical Appearance | White, crystalline solid |
| Melting Point | Decomposes at 459 K |
What is the molar mass of Na2SO4 quizlet?
In the example, the molar mass of Na2SO4 is (23 x 2) + (32 x 1) + (16 x 4) = 142 grams per mole.
How many moles of NaOH are in 8.00 g?
The number of moles of the NaOH sample is 0.20.
What is the mass of 0.25 moles of water?
5gm
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What is mercury (II) bromide?
This white solid is a laboratory reagent. Like all mercury salts, it is highly toxic. Mercury (II) bromide can be produced by reaction of metallic mercury with bromine.
How do you make Mercury bromide from mercuric salt?
Mercury(II) bromide can be manufactured by: adding potassium bromide to a solution of mercuric salt and crystallizing; by precipitation using a mercury(II) nitrate and sodium bromide solution; by dissolving mercury(II) oxide in hydrobromic acid.
What is the molar mass of Hg (NO3) 2?
Molar mass of Hg(NO3)2 = 324.5998 g/mol. Convert grams Mercury(II) Nitrate to moles or moles Mercury(II) Nitrate to grams.
What happens when arsenic is added to mercury (II) bromide?
The white mercury (II) bromide will turn yellow, brown, or black if arsenic is present in the sample. Mercury (II) bromide reacts violently with elemental indium at high temperatures and, when exposed to potassium, can form shock-sensitive explosive mixtures.