Best Answer

From the Periodic Table

The Atomic Mass of Nitrogen (N) is 14

The Atomic mass of Oxygen (O) is 16

Hence the gram formula mass of NO is 14 + 16 = 30

Now NO under certain circumstances can form N2O2 hence the gram formula mass of N2O2 = (2 x 14) + ( 2 x 16) = 28 + 32 = 60

However the empirical formula is the formula with the lowest ratio of atoms. Hence N2O2 lowest ration is NO # formula mass is 30 .

Study guides

☆☆

Q: Why can't a substance have an empirical formula of NO and a gram formula mass of 45g?

Write your answer...

Submit

Still have questions?

Continue Learning about Natural Sciences

the answer is: P4O10

The gram molecular mass of the molecule must be measured by some independent method such as freezing point depression or boiling point elevation. Then the factor by which to multiply all of the subscripts in the empirical formula to get the molecular formula is the closest integer to the ratio of gram molecular mass to the gram molecular mass of a single unit of the empirical formula.

To find empirical formulas from mass data such as are presented in this question, first convert the masses given to gram atoms by dividing the stated mass for each element by the gram atomic mass of the element. For aluminum, 3.704/26.9815 is about 0.137279; for oxygen, 3.295/15.9994 is about 0.205945. Then divide the larger of these numbers of gram atoms by the smaller to produce a quotient of 1.500. The smallest integers that approximate this ratio are 3 and 2. Therefore, the empirical formula is Al2O3.

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.

Calcium oxide is CaO.

Related questions

C8h18

the answer is: P4O10

The gram formula unit mass of the empirical formula C2H3 is twice the gram atomic mass of carbon plus three times the gram atomic mass of hydrogen, or about 27. The nearest integer to 162.27/27 is 6. Therefore, the molecular formula for the compound is C12H18.

The gram molecular mass of the molecule must be measured by some independent method such as freezing point depression or boiling point elevation. Then the factor by which to multiply all of the subscripts in the empirical formula to get the molecular formula is the closest integer to the ratio of gram molecular mass to the gram molecular mass of a single unit of the empirical formula.

To find empirical formulas from mass data such as are presented in this question, first convert the masses given to gram atoms by dividing the stated mass for each element by the gram atomic mass of the element. For aluminum, 3.704/26.9815 is about 0.137279; for oxygen, 3.295/15.9994 is about 0.205945. Then divide the larger of these numbers of gram atoms by the smaller to produce a quotient of 1.500. The smallest integers that approximate this ratio are 3 and 2. Therefore, the empirical formula is Al2O3.

The molecular formula of this compound is N2H2. This is obvious because the empirical formula of a compound is the lowest positive integer ratio of atoms present.

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.

By first determining the approximate molecular mass of the compound in question, usually by measurements of osmotic pressure, freezing point depression, or some other colligative property that depends on the number of molecules present. The approximate molecular mass of the substance in question is then calculated from the colligative property measurements, and this value is then divided by gram molecular mass corresponding to the empirical formula. The nearest integer to the resulting quotient is then applied as a factor by which to multiply each subscript of the empirical formula to yield the molecular formula.

by determining its gram formula mass

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 gram formula mass

A gram of a molecular substance is the quantity that will have a mass of 1 gram.

People also asked