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The actual molar ratio of elements in a compound as expressed by the subscripts in a formula is expressed in what?
The actual molar ratio of elements in a compound as expressed by the subscripts in a formula is the formula unit. It represents the simplest whole-number ratio of atoms of each element in the compound.
What molecular formulas are an empirical formula?
Any molecular formula where the subscripts do not have a common factor that can divide them all. For example: CH4 (methane) is a molecular formula that is also an empirical formula because there is no number (other then one) that can divide both the 4 and the 1. Take ethane as another example. It hasn't the empirical formula which is similar to the molecular formula.
What is the empirical formula of a compound with the molecular formula C 12 H 8?
The empirical formula of a compound with the molecular formula C12H8 is CH2. This is determined by dividing the subscripts in the molecular formula by the greatest common factor (in this case, 4) to obtain the simplest whole-number ratio of atoms in the compound.
What is an emperical formula?
An empirical formula represents the simplest whole-number ratio of atoms in a compound. It does not provide information about the actual number of atoms present in a molecule. To determine the empirical formula, one must divide the subscripts of the compound's molecular formula by the greatest common divisor to obtain the simplest ratio.
How to calculate empirial formula from molecular formula?
To calculate the empirical formula from a molecular formula, divide the subscripts in the molecular formula by the greatest common factor to get the simplest ratio of atoms. This simplest ratio represents the empirical formula.
What is Na2S2O4 formula is empirical formulas?
The empirical formula of Na2S2O4 is NaSO2. This is determined by dividing the subscripts in the molecular formula by their greatest common factor to obtain the simplest whole-number ratio of atoms present in the compound.
How can one learn how to read a molecular formula effectively?
To effectively read a molecular formula, one can start by understanding the symbols used to represent elements and the subscripts that indicate the number of atoms of each element in the compound. Practice identifying elements and their corresponding symbols, and interpreting the subscripts to determine the ratio of atoms in the compound. Additionally, familiarize yourself with common prefixes and suffixes used in naming compounds to help decipher the molecular formula. Regular practice and exposure to different molecular formulas will improve your ability to read them effectively.
What is the chemical formula of a molecular compound called?
The chemical formula of a molecular compound represents the types and numbers of atoms in a molecule. It is derived by writing the symbols of the constituent elements in the compound and indicating the number of atoms of each element using subscripts.
What is the difference between empirical and molecular formula?
An empirical formula is one that shows the lowest whole number ratio of the elements present. The molecular formula shows the composition of the molecules. An example is phosphorus pentoxide, P2O5 empirical formula, P4O10 molecular formula.
Are prefixes not considered when writing formulas for molecular componds?
Yes, prefixes are not considered when writing formulas for molecular compounds. The subscripts in a molecular formula represent the ratio of atoms in the compound without taking into account any prefixes used to indicate the number of each element.
What is the empirical formula for K3PO4?
The empirical formula for K3PO4 is K3PO4 itself. This is because the subscripts in the formula (3 for potassium, 1 for phosphorus, and 4 for oxygen) represent the simplest whole-number ratio of the elements in the compound.
How do you calculate Molecular formula from empirical formulaWhat could you do with that information to determine that the empirical and molecular formulas are related to one another by a factor of 6?
In order to find molecular formula from empirical formula, one needs to know the molar mass of the molecular formula. Then you simply divide the molar mass of the molecular formula by the molar mass of the empirical formula to find out how many empirical formulae are in the molecular formula. Then you multiply the subscripts in the empirical formula by that number.
