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What is the gram mass of compound if 5 moles of the compound has a mass of 100 grams?
Wiki User
∙ 10y ago
The molar mass is 20 g.
Wiki User
∙ 7y ago
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Formula for moles?
number of moles = mass of the material/molar mass
What is the mass of 2.47 moles of fluorine atoms?
The gram atomic mass of fluorine is 18.9984. Therefore, the mass of 2.47 moles is 2.47 times the gram atomic mass, or about 46.9 grams, to the justified number of significant digits.
How many grams are there in 3.3 x 1023 moles?
This depends on the molar mass of the compound involved.
Grams per liter into moles per liter how to convert?
divide by the molecular mass, (units of gram per mol)
A sample of cinnamaldehyde C9H8O contains 0.0976 mol of the compound What is the mass off the sample in grams?
Multiply the number of moles (0.0976) by the molar mass of C9H8O (9*12.0+8*1.008+16.0= 132.1) in units: moles * grams/mole = grams
What do you do to convert grams to moles?
The molar mass of a compound is expressed in grams.
What is the mass in grams of 8.56 moles?
This depends on the compound.
Formula for moles?
number of moles = mass of the material/molar mass
Which statement shows how to correctly convert from the mass of a compound in grams to the amount of that compound in moles?
Moles = Mass (g) x Molar mass (g)
How many moles of carbon dioxide are in 418 grams of the compound?
The gram molecular mass of carbon dioxide is 44.01. Therefore, 418 grams contains 418/44.01 or 9.50 moles, to the justified number of significant digits.
What is the mass of kbr in 2.50 moles of the compound?
The mass number of potassium is about 39. The mass number of bromine is about 80. Total is 119. 119* 2.5 = 297.5. So 297.5 grams of potassium bromide has got 2.5 gram moles.
How many moles of CCl4 are present in 22.5 g of the compound?
For this conversion, you need the atomic masses of the elements involved, found on any periodic table. Then you add them up with their abundance in the compound to find the total molar (molecular) mass. The molar mass is the mass in grams of one mole of the compound. Carbon = 12.0 grams Chlorine = 35.5 grams × 4 atoms = 142.0 grams ------------------------------------------------------------- Carbon tetrachloride = 154.0 grams/mole Then you do a gram --> mole conversion, taking the amount given and dividing it by the molar mass. Grams ÷ Molar mass = Moles 22.5 grams ÷ 154.0 grams = 0.146 moles CCl4
How do you calculate moles to grams?
Chemical Engineers sometimes measure substance amount in units of gram-moles, kilogram-moles, pound-moles, or ounce-moles; these measure the quantity of a substance whose molecular weight is not equal to its mass in grams, kilograms, pounds, or ounces. The SI mole is identical to the gram-mole. This is from wikipedia entry on moles. So 1 mole = 1 gram-mole
What is the mass of 2.47 moles of fluorine atoms?
The gram atomic mass of fluorine is 18.9984. Therefore, the mass of 2.47 moles is 2.47 times the gram atomic mass, or about 46.9 grams, to the justified number of significant digits.
0.871 moles is how many grams?
Multiply the number of moles by the molecular weight of the compound (or atomic weight for an element) to find the mass in grams.
How many moles are there in a 2.0g sample of NaCl?
Strictly, the compound NaCl does not have "moles", because the compound is ionically bonded. The gram formula unit mass, which is substituted for molar mass for ionic compounds, is 58.44, and 2.00 g of NaCl therefore contains 2.00/58.44 or 3.42 X 10-2 gram formula units.
What is the type of conversion factor needed in a problem in which mass is being converted to moles?
moles to atoms you multiply the number of moles by avogadros number ex: 1.32 mol x (6.022 x 10^23 atoms)/mol mass to atoms you multiply the mass (in grams) times the molar mass of the element or compound (ex: N 14.01 mols/gram) then times avogadros number once you have the moles. ex: 45.6 g N x (14.01 mol/gram) x (6.022 x 10 ^23 atoms/mol) if it's a compound instead of an element, find the molar mass of the compound (the molar masses of all the elements in it added up) and multiply by it. ------------------------- Actually you are wrong, from mass to atoms you need to take the initial mass divide by the gram of the element that you are doing and multiply by the Avogadros number
