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A compound is 40.0 C 6.70 H and 53.3 O by mass what is subscript of empirical formula?
Wiki User
∙ 14y ago
c=1
H=2
O=1
Wiki User
∙ 14y ago
To determine the subscript of the empirical formula, you first need to calculate the molar mass of the compound using the given percentages. Then, divide the molar mass of the compound by the molar mass of each element (12.01 g/mol for C, 1.01 g/mol for H, and 16.00 g/mol for O). Finally, divide the resulting values by the smallest value obtained to get the simplest ratio of elements in the compound, which will give you the subscript of the empirical formula.
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To determine the subscript of an element in a molecular formula the empirical mass must be multiplied by the actual mass?
Determining the subscript of an element in a molecular formula involves comparing the actual mass of the element with its empirical mass, then dividing the actual mass by the empirical mass to find the subscript. This calculation helps to determine the ratio of atoms of a particular element in a compound.
The analysis of an organic compound showed that it contains 0.175 mol C 0.140 mol H and 0.035 mol N. Its molecular mass is about 160 gmol. What is the subscript on C in the chemical formula?
The compound's empirical formula is CH3N, and its molecular formula is C4H12N. Therefore, the subscript on C in the chemical formula is 4.
How does one determine a molecular formula from the empirical form?
To determine the molecular formula from the empirical formula, you need the molar mass of the compound. Divide the molar mass of the compound by the molar mass of the empirical formula to find the "n" constant. Then, multiply the subscripts in the empirical formula by the "n" constant to get the molecular formula.
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.
To determine the subscript of an element in a molecular formula the empirical mass must be multiplied by the actual mass?
Determining the subscript of an element in a molecular formula involves comparing the actual mass of the element with its empirical mass, then dividing the actual mass by the empirical mass to find the subscript. This calculation helps to determine the ratio of atoms of a particular element in a compound.
What steps are used to convert an empirical formula into a molecular formula?
By determining the molecular mass, then dividing the molecular mass by the formula mass of the empirical formula to determine by what integer the subscripts in the empirical formula must be multiplied to produce the molecular formula with the experimentally determined molecular mass.
What is the properly written empirical formula of a compound of molecular formula C6H12 with a molar mass equal to 84.16 gram per mol?
The information about the actual molar mass is superfluous. Given any molecular formula, the corresponding empirical may be obtained by dividing all the subscripts in the molecular by the largest integer that yield an integer quotient for each subscript. In the given formula, the empirical formula is CH2.
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.
If a compound containing chromium and silicon has 73.52 mass percent chromium what is its empirical formula?
To find the empirical formula, we need to determine the molar ratio of chromium to silicon. If 73.52% of the compound's mass is chromium, then the mass of silicon must be 100% - 73.52% = 26.48%. Next, we convert these percentages to moles, then divide by the smallest number of moles to get the simplest whole number ratio. The empirical formula is CrSi.
What information is given by a molecular formula?
the empirical formula and the molar mass
What is the molecular formula of a compound with the empirical formula C13H19O2 and molar mass of 414.64g?
The molar mass of the compound is 414.64 g/mol. The empirical formula is C13H19O2, which has a molar mass of 13 x 12.01 g/mol + 19 x 1.01 g/mol + 2 x 16.00 g/mol = 203.32 g/mol. To calculate the molecular formula, divide the molar mass of the compound by the molar mass of the empirical formula: 414.64 g/mol / 203.32 g/mol = 2.04. Therefore, the molecular formula is approximately 2 times the empirical formula, which is C26H38O4.
What is the molecular formula of a compound given that molar mass of the compound is 30.04 gram and the empirical formula is NH?
The molar mass of ammonia (NH) is approximately 17.03 g/mol. To get a molar mass of 30.04 g/mol, we need to determine how many times the empirical formula must be multiplied by a whole number. 30.04 / 17.03 ≈ 1.76, so the molecular formula would be NH₂.
What is this empirical formula - C5H8NO4?
C4h5n2o
The empirical formula of a compound is ch2its molecular mass is 70 gmol what is its molecular formula?
C5h10
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.
The mole establishes a relationship between the?
the molecular mass of a compound and its empirical formula
