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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 .

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lenpollock

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โˆ™ 2023-02-02 17:02:11
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Q: Why can't a substance have an empirical formula of NO and a gram formula mass of 45g?
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Continue Learning about Natural Sciences

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the answer is: P4O10


How the moleculer formula of a compound is calculated if its emperical formula is known?

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.


What is the empirical formula of a substance that consists of 3.704g aluminum and 3.295g oxygen?

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.


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.


If A 2.50-gram sample of calcium metal is heated in a 38.500 gram crucible to form a calcium oxide. if the crucible and product weigh 38.850 g what is the empirical formula for calcium oxide?

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Related questions

What is the molecular formula of a compound with an empirical formula of C4H9 and a gram formula mass of 114 grams mole?

C8h18


What is the molecular formula of a compound with the empirical formula P2O5 and a gram-molecular mass of 284 grams?

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What is the molecular formula of a compound given the molar mass of the compound is 162.27 grams and the empirical formula is C2H3?

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.


How the moleculer formula of a compound is calculated if its emperical formula is known?

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.


What is the empirical formula of a substance that consists of 3.704g aluminum and 3.295g oxygen?

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.


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 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.


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.


How does one determine the molecular formula from the empirical formula?

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The mass of a mole of a substance is equal to?

by determining its gram formula 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?

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What is the mass in grams of one mole of any pure substance?

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