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Would you expect an empirical formula to be the same even though different masses used?
Wiki User
∙ 12y ago
This question refers to masses of elements as opposed to their molecular formulas. In the example of MgCl2 there will always be Mg in a 1:2 molar ratio with chlorine. Molar mass gives the relationship.
Wiki User
∙ 9y ago
Wiki User
∙ 12y agoYes, if we're talking about different masses of the same compound.
This is because an empirical formula is the simplest whole number ratio of elements in a compound.
For example water contains 2 hydrogen atoms for every one oxygen atom.
If I have 18 grams of water, I have 2 mol H and 1 mol O. The empirical formula is H2O.
If I have 36 grams of water, I have 4 mol H and 2 mol O. 4:2 simplifies to 2:1. The empirical formula is still H2O.
If I find another compound of hydrogen and oxygen, and it has 1 mol hydrogen for every 1 mol oxygen, the empirical formula is HO, and this new compound is NOT water.
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How many different masses of the Cl2 molecule would you expect to find in a sample of chlorine gas?
three different masses.
What is the empirical formula for 16 grams of sulfur reacting with 24 grams of oxygen?
To find empirical formulas, masses of elemental reactants must be changed to gram atoms by dividing the mass by the gram atomic masses of each element. Thus, 16 grams of sulfur constitutes 16/32.06 or 0.50 mole to the justified number of significant digits, and 24 grams of oxygen constitutes 24/15.9994 or 1.50 moles of oxygen to the justified number of significant digits. Therefore, the atomic ratio of oxygen to sulfur in the compound is 1.50/0.50 or 3, and the empirical formula is SO3.
What is the empirical formula for a molecule containing 46.8 Si and 53 O?
This compound is silicon dioxide - SiO2.
Empirical formula of a compound that contains 85.6 percent carbon and 14.4 percent?
Hypothetically, 100g of this substance will contain 52.1 g carbon, 13.2 g hydrogen and 34.7 g oxygen. Dividing these by their respective molar masses gives the amount in moles of each element. These are 4.34 mol, 13.1 mol, and 2.17 mol respectively. Divide all amounts given by the smallest non-integer amount, then multiply by whole numbers until the simplest ratio is found. These are 2 mol, 6 mol, and 1 mol respectively. The empirical formula of ethanol is C2H6O.
What is the sum of the atomic masses of all the atoms in a molecule?
molecular mass
Use the masses of carbon dioxide CO2 and water H2O to determine the empirical formula of the alkane component?
C3h7
How many different masses of the Cl2 molecule would you expect to find in a sample of chlorine gas?
three different masses.
How is the formula of hydrogen gas different from the formula for helium gas?
the answer is simple it is that both elements have different masses which makes each formula different
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 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 does an empirical formula show?
the empirical formula of a compound tells you the proportions of the elements in the compound. with that information you can make some inferences about the identity of the compound. for example a compound with an empirical formula CH4 tells us that for every carbon atom there are four hydrogen atoms. this means that the compound is methane because no other hydrocarbon can have these roportions (try drawing the lewis structure for C2H8, which doesnt exist. you cant!)
How do you determine the molecular formula of a compound from its empirical formula?
If you are given the empirical formula and are asked for the actual formula, then the molecular mass of the compound will be given too. Take this example problem: Empirical Formula: CH2O Molecular Mass: 180.0 First you have to find the empirical mass. Just find the atomic masses of all the elements in the empirical formula and add them together. If there are multiple atoms of the same element, then you have to add the element's atomic mass for every multiple. In the example, you have to add hydrogen twice because there are two hydrogen atoms in the empirical formula. C- 12.0 H- 1.00 H- 1.00 O- 16.0 + _________ 30.0 The empirical formula is some multiple of the actual formula. The empirical formula shows the ratio of atoms as 1:2:1. This means that the actual formula could be 2:4:2 or 3:6:3 or 4:8:4 etc. In order to find what multiple it is, divide the molecular mass by the empirical mass. An easier way to think of it is: x(empirical mass) = molecular mass Use this formula to find x: x(30.0) = 180.0 x = 6 In this example, x turned out to be exactly 6, but in some cases (especially in lab results) the answer will be close to a whole number but not exact. There is usually a standard +/- .02 for your result. If the x value was 6.02 or 5.98, we would just round up or down as long as it is within .02 Take the x value and multiply it with the number of atoms in the original empirical formula. C1H2O1 * 6 = C6H12C6 The final result is the actual molecular formula.
What is the empirical formula for 16 grams of sulfur reacting with 24 grams of oxygen?
To find empirical formulas, masses of elemental reactants must be changed to gram atoms by dividing the mass by the gram atomic masses of each element. Thus, 16 grams of sulfur constitutes 16/32.06 or 0.50 mole to the justified number of significant digits, and 24 grams of oxygen constitutes 24/15.9994 or 1.50 moles of oxygen to the justified number of significant digits. Therefore, the atomic ratio of oxygen to sulfur in the compound is 1.50/0.50 or 3, and the empirical formula is SO3.
What is the empirical formula for a molecule containing 46.8 Si and 53 O?
This compound is silicon dioxide - SiO2.
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 meant by law of constant proportion and how is this law applied in experiment empirical formula of a compound?
The law of constant proportion states that a pure chemical compound always contains exactly the same proportion of elements by mass.This information, together with the atomic masses of the elements in the compound enable scientists to determine the formula of a compound.
Empirical formula of a compound that contains 85.6 percent carbon and 14.4 percent?
Hypothetically, 100g of this substance will contain 52.1 g carbon, 13.2 g hydrogen and 34.7 g oxygen. Dividing these by their respective molar masses gives the amount in moles of each element. These are 4.34 mol, 13.1 mol, and 2.17 mol respectively. Divide all amounts given by the smallest non-integer amount, then multiply by whole numbers until the simplest ratio is found. These are 2 mol, 6 mol, and 1 mol respectively. The empirical formula of ethanol is C2H6O.
