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A sample of a compound contain 1.52 g of Nitrogen and 3.47 g of Oxygen. The molar mass of this compound is between 90 grams and 95 grams. Determine molecular formula and the accurate molar mass.?
A sample of a compound contain 1.52 g of Nitrogen and 3.47 g of Oxygen. The molar mass of this compound is between 90 grams and 95 grams. The molecular formula and the accurate molar mass would be N14O35.
The actual molar ratio of elements in a compound as expressed by the subscripts in a formula is expressed in what?
The actual molar ratio of elements in a compound as expressed by the subscripts in a formula is the formula unit. It represents the simplest whole-number ratio of atoms of each element in the compound.
A compound with the empirical formula SN was found in a subsequent experiment to have a molar mass of 184.32 gmol. What is the molecular formula of the compound?
The empirical formula of SN has a formula unit mass of the sum of the gram atomic masses of nitrogen and sulfur, i.e., about 46.0667. The gram molecular mass given in the problem divided by this formula unit mass is about 4. Therefore, the molecular formula is S4N4.
What is the molecular formula of the compound CH with molar mass 42.0?
The molecular formula of the compound CH with a molar mass of 42.0 g/mol is C3H3. This can be calculated by dividing the molar mass by the molar mass of a carbon atom (12 g/mol) to determine the number of carbon atoms, and then assigning the remaining mass to hydrogen atoms.
Determine the molecular formula of a compound if its empirical formula is C2H6O and its molar mass is 138g?
Because an empirical formula is the simplest form of a compound, we know that the molecular formula contains more atoms than it does. Since we are given the molar mass, we can use this formula. x ( MM of empirical formula ) = MM of molecular formula MM of empirical formula = 12(2) + 1(6) + 16 = 46 MM of molecular formula = 138 46x = 138 x= 138 / 46 x=3 Therefore, the molecular formula is 3(C2H6O) that is C6H18O3
What is the molecular formula of a compound with the empirical formula NH2Cl and molar mass of 51.5g mol?
The empirical formula NH2Cl has a molar mass of 51.5 g/mol, so the molecular formula can be determined by finding the ratio of the molar mass of the molecular formula to the molar mass of the empirical formula. The molecular formula of the compound is therefore NH2Cl2.
How do you find molecular fomula?
To find the molecular formula of a compound, you need to know its empirical formula and molar mass. Divide the molar mass of the compound by the molar mass of the empirical formula to find the "multiplication factor." Multiply the subscripts in the empirical formula by this factor to get the molecular formula.
What is the molecular formula of the compound CH2 with molar mass = 42.0?
The molecular formula of a compound can not be determined solely based on its molar mass. In this case, without additional information, it is not possible to determine the molecular formula of the compound CH2.
How does one determine a molecular formula from the empirical form?
molar mass of unknown/molar mass of empirial = # of empirical units in the molecular formula. Example: empirical formula is CH2O with a molar mass of 30. If the molar mass of the unknown is 180, then 180/30 = 6 and molecular formula will be C6H12O6
What is the molecular formula of the compound CH2 with a molar mass 42.0 gmol?
The molecular formula of the compound is C2H4, which has a molar mass of 28 g/mol. Since the given compound has a molar mass of 42.0 g/mol, it must include an additional CH2 group, resulting in the molecular formula C2H6.
What is the molecular formula of the compound CH2 with molar mass equals 168?
The molecular formula of the compound CH2 with a molar mass of 168 is C7H14. This molecular formula satisfies the condition of having two hydrogen atoms bonded to each carbon atom, resulting in a molar mass of 168 g/mol.
What is the molecular formula of a compound that has the molar mass of 207?
Without further information, it's not possible to determine the molecular formula of a compound just from its molar mass. Additional details about the elements present and their respective ratios are needed to ascertain the specific molecular formula.
What is the molecular formula of the compound CH2 with molar mass 168 gmol?
c12h24
What is the molecular formula of a compound containing 89 cesium (Cs) and 11 oxygen (O) with a molar mass 298 gmol?
The molar mass of the compound is 298 g/mol. To find the molecular formula, we need to calculate the molar mass of Cs and O; Cs has a molar mass of approximately 132.91 g/mol, and O has a molar mass of approximately 16 g/mol. Using these values, we can determine that the compound's molecular formula is Cs11O11.
What is the molecular formula of compound CH2 with a molar mass of 42.0?
The molecular formula of compound CH2 with a molar mass of 42.0 g/mol is C2H4, which is ethylene. Each carbon has a molar mass of 12.0 g/mol, and each hydrogen has a molar mass of 1.0 g/mol, totaling 42.0 g/mol.
A compound has a mass of 16.7g 12.7g Iodine 4g Oxygen Therefore the empirical formula is I2O5 What additional information do you need to work out the molecular formula?
To determine the molecular formula, you would need the molar mass of the compound. With the molar mass, you can calculate the empirical formula mass and then determine the ratio between the empirical formula mass and the molar mass to find the molecular formula.
The empirical formula of a compound is CH2O The molar mass of the compound is 180 g What is the molecular formula for this compound?
The empirical formula CH2O has a molar mass of 30 g/mol (12 g/mol for C + 2 g/mol for H + 16 g/mol for O). To find the molecular formula, which is a multiple of the empirical formula, you divide the molar mass given (180 g/mol) by the empirical formula mass (30 g/mol), giving you 6. Therefore, the molecular formula for the compound is (CH2O)6, which simplifies to C6H12O6, the molecular formula for glucose.
