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What is the empirical formula for a compound if a 20.0 g sample contains 4.0 g Ca and 16.0 g Br?
CaBr2
What song did biggie sample for nasty boy?
Contains a sample of "Cavern" by Liquid Liquid
What sample is used for the song players by slum village?
the song is Clair by the singers unlimited Formula for total work?
What does kid cudi say at the beginning of mojo so dope?
"Mojo So Dope" contains a sample of "Claustrophobia" by Choir of Young Believers.
What Dubstep tune has the sample from Chopper in it?
The one that has a sample of chopper in it.
empirical formula of a 9.50g sample of a compound that contains 3.03g of K 2.75g Cl and O?
This compound is potassium oxide, K2O.
What is the empirical formula for a compound if a 20.0 g sample contains 4.0 g Ca and 16.0 g Br?
CaBr2
What is the empirical formula of a compound composed of 31.1 g potassium and 6.36 g oxygen?
The molar mass of potassium is 39.10 g/mol and the molar mass of oxygen is 16.00 g/mol. To find the empirical formula, we first need to convert the masses to moles: 31.1 g K is 0.797 mol K and 6.36 g O is 0.3975 mol O. Then, we divide each mole value by the smallest mole value to get the mole ratio, which gives us K2O as the empirical formula.
What is the empirical formula if a 100.0 g sample of a compound is composed of 16.3 g of carbon 32.1 g of chlorine and 51.6 g of fluorine?
To find the empirical formula, convert the masses of each element to moles. The molar ratio of carbon to chlorine to fluorine is 1:1:2. Therefore, the empirical formula is CClF2.
A sample of titanium with a mass of 1.10 g was heated and completely reacted with chlorine gas. The resulting compound had a mass of 3.54 g. What is the empirical formula of the chloride that formed?
To find the empirical formula, you first need to determine the moles of titanium and chlorine in the compound. The molar mass of titanium is 47.87 g/mol, and chlorine is 35.45 g/mol. From the given masses, you can calculate the moles of titanium and chlorine in the compound. Then, divide the moles by the smallest number of moles to get the mole ratio for the empirical formula. In this case, the empirical formula of the chloride formed is TiCl3.
An unknown sample with a molecular mass of 180.0g is analyzed to yield 40 percent C 6.7 percent H and 53.3 percent O What is the empirical formula and the molecular formula of this compound?
The empirical formula is CH2O. To find the molecular formula, you need to calculate the empirical formula weight (30 g/mol) and divide the molecular mass (180.0 g/mol) by the empirical formula weight to get 6. This means the molecular formula is (CH2O)6, which simplifies to C6H12O6, the molecular formula of glucose.
What is the empirical formula of an oxide of Bromine which contains 71.4 percent Bromine by mass?
The empirical formula of the oxide of Bromine would be Br2O5. We can determine this by assuming a 100 g sample, which would contain 71.4 g of Bromine and 28.6 g of Oxygen. Then we convert these masses into moles and divide by the smaller value to find the mole ratio, which gives the empirical formula.
A 7.300 gram sample of aluminum was quantitatively combined with a sample of selenium to form a compound The compound weighed 39.35 grams What is the empirical formula for this compound?
The molar mass of aluminum is 26.98 g/mol, and the molar mass of selenium is 78.96 g/mol. Using the given masses, we find that there are 0.270 moles of aluminum and 0.499 moles of selenium in the compound. Dividing by the smallest number of moles (0.270) gives us the empirical formula Al2Se3.
Determine the empirical formula what compound if a sample contains 0.104 mol K 0.052 mol C and 0.156 mol O?
To find the empirical formula, we need to determine the ratio of each element in the compound. First, find the moles of each element: K = 0.104 mol C = 0.052 mol O = 0.156 mol Next, divide each mole value by the smallest mole value to get the ratio: K = 0.104 mol / 0.052 mol = 2 C = 0.052 mol / 0.052 mol = 1 O = 0.156 mol / 0.052 mol = 3 Therefore, the empirical formula is K2CO3.
How To Determine The Empirical Formula From 46.25 grams Sample That Contains 14.77 grams Of K 9.06 Of O 22.42 grams Of tin.?
To determine the empirical formula, first calculate the moles of each element present by dividing the given masses by their respective molar masses. Then, divide each mole value by the smallest mole value obtained. Finally, round the resulting ratio to the nearest whole number to determine the subscripts required for the empirical formula. In this case, the empirical formula would be K2O2Sn.
Determine the empirical formula of the following compound if a sample contains 5.28g Sn and 3.37g F?
To determine the empirical formula, first convert the grams of each element to moles by dividing by their respective molar masses. Next, find the ratio of moles of each element to each other. Finally, divide by the smallest number of moles to get a whole number ratio. In this case, the empirical formula is SnF2 as the ratio of moles of Sn to F is 1:2.
What three types of information are needed on order to find an empirical formula from percentage composition data?
· Assume that you have 100.0 g sample of the compound · Calculate the amount of each element in the sample · Convert the mass composition of each element to a composition in moles by dividing by the appropriate molar mass
