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Is the empirical formula molar mass less than or equal to the actual molar mass for all compound?
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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.
What is its empirical formula isooctane?
I don't know the exact formula but, i know the density of iso-octane: 0.69 g/ml And one gallon is equal to 3,840 ml so.... all you need is the volume.
Do the Empirical formula relates the mass of each element in a compound to the entire mass of the compound?
An empirical formula gives this information indirectly by specifying the ratios of numbers of atoms of each element in a compound to the total number of atoms in a compound. These ratios can then be mathematically converted into the mass ratios specified in the question by using the known atomic weights of each element present: The mass ratio of element "Q" to element "R" is equal to the number ratio multiplied by the ratio of the atomic weight of element Q to that of element R. For example, the number ratio of hydrogen to oxygen in water is 2, but the mass ratio is 2(1.008/15.999) = 0.1260.
What do images of atoms and molecules show?
The empiracle formula shows the ratio of the individual elements in a compound, and the molecular formula shows the actual number of each elemental atom in each molecule (which will be equal to the empiracle formula or a whole number multiple of it). However, it is the structural formula that shows how the individual atoms are connected.
What is the molecular formula of a compound with an empirical formula of C2OH4 and a molar mass of 88 grams per mole?
Look at your atomic masses for phosphorus and oxygen. Set up 2.5/31 and 3.23/16. This makes 0.08 and 0.2. Now consider 0.08/0.2 to equal 0.4. So, your ratio of P to O is 0.4, which is 4/10. So, your formula, which reflects that ratio, is P4O10. That's tetraphosphorus decoxide, a molecular solid used in match-heads.
What is the empirical formula of the compound that is 75 carbon and 25 hydrogen?
The empirical formula of a compound is the simplest whole number ratio of the elements in the compound. In C75H25, the ratio of carbon to hydrogen is 75:25, which is equal to 3:1. Thus, the empirical formula is C3H.
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.
Is the number of atoms in a molecular formula always greater than a empirical?
No. A molecular formula can be the same as the empirical formula, such as CH4 (methane), because the two component atoms exist in a ratio that cannot be mathematically further broken down - one carbon to four hydrogens. In this case the molecular formula (the actual number of atoms per molecule), and the empirical formula (the simplest ratio of those numbers) is identical. On the other hand, ethane, C2H6 - two carbons to 6 hydrogens - has a molecular formula of C2H6 and a empirical formula of CH3, the ratio of 2 to 6 reduced to its simplest whole number form. Sooooooooooo, the molecular formula will always be equal to or greater than the empirical formula, and the empirical formula will always be equal to or less than the molecular formula. In other words (as if that wasn't enough), the molecular formula will never be less than the empirical formula and the empirical formula will never be greater than the molecular formula, but THE TWO CAN BE EQUAL. Whew!!! Ray
Does no and no2 have the same empirical formulas?
No: The formula NO shows equal numbers of nitrogen and oxygen atoms in the compound, but the formula NO2 shows twice as many oxygen atoms as nitrogen atoms.
What is an empirical formula?
The chemical formula in which the subscripts are given in the smallest ratio.
How do you find the molecular and empirical formulas?
There is no easy answer to this question. First, it depends what information you have to start with. Do you have the name? Do you know what elements are found in the substance?If you are given the name of the molecule, you can often find the molecular structure of that compound by simply using the Google search engine online and searching for the name. It is often give you the answer! There are certain compounds that you should be familiar with also. Also, there is a set of official rules that determine the name of a specific compound, so that if you have the formula, you can name it correctly, and if you have the name, you can determine the formula. Unfortunately, many chemicals also have common names that do not follow these rules, and you just have to memorize those, or look them up with Google.See the Related Questions and Web Links to the left for some information about how compounds are named and how to go from a formula to a name and vice versa.
What is the formula of the compound formed by potassium and chloride?
The formula is KCl. This is an ionic compound consisting of equal numbers of potassium cations and chloride anions.
What is its empirical formula isooctane?
I don't know the exact formula but, i know the density of iso-octane: 0.69 g/ml And one gallon is equal to 3,840 ml so.... all you need is the volume.
Do the Empirical formula relates the mass of each element in a compound to the entire mass of the compound?
An empirical formula gives this information indirectly by specifying the ratios of numbers of atoms of each element in a compound to the total number of atoms in a compound. These ratios can then be mathematically converted into the mass ratios specified in the question by using the known atomic weights of each element present: The mass ratio of element "Q" to element "R" is equal to the number ratio multiplied by the ratio of the atomic weight of element Q to that of element R. For example, the number ratio of hydrogen to oxygen in water is 2, but the mass ratio is 2(1.008/15.999) = 0.1260.
What do images of atoms and molecules show?
The empiracle formula shows the ratio of the individual elements in a compound, and the molecular formula shows the actual number of each elemental atom in each molecule (which will be equal to the empiracle formula or a whole number multiple of it). However, it is the structural formula that shows how the individual atoms are connected.
What are the sum of atomic masses of all atoms formula for a compound called?
It is called the molar mass of that compound. In other words, the total mass of all of the elements in a compound is equal to one mole of that compound.
What is the molecular formula of a compound with an empirical formula of C2OH4 and a molar mass of 88 grams per mole?
Look at your atomic masses for phosphorus and oxygen. Set up 2.5/31 and 3.23/16. This makes 0.08 and 0.2. Now consider 0.08/0.2 to equal 0.4. So, your ratio of P to O is 0.4, which is 4/10. So, your formula, which reflects that ratio, is P4O10. That's tetraphosphorus decoxide, a molecular solid used in match-heads.
