0
molar mass is the Atomic Mass of the element. it's on the Periodic Table. you just have to add them up. unless you want to calculate the number of moles in a compound, in that case: moles = mass/molar mass
What else can I help you with?
How do you find the percent of oxygen by mass in a compound?
To find the percent of oxygen by mass in a compound, you need to know the molar mass of the compound and the molar mass of oxygen. Divide the molar mass of oxygen by the molar mass of the compound and multiply by 100 to get the percentage.
What is the percentage composition of molar mass in the given compound?
The percentage composition of molar mass in a compound is the percentage of each element's mass contribution to the total molar mass of the compound.
What is the molar mass of the nonelectrolyte compound if a 4.305 g sample of it is dissolved in 105 g of water?
To find the molar mass of the nonelectrolyte compound, we need to use the formula: Molar mass (mass of compound / moles of compound) First, we need to find the moles of the compound by using the formula: moles mass / molar mass Given that the mass of the compound is 4.305 g and it is dissolved in 105 g of water, we can calculate the moles of the compound. Next, we can find the molar mass of the compound by rearranging the formula: Molar mass mass / moles By plugging in the values, we can calculate the molar mass of the nonelectrolyte compound.
What is the molecular formula of the compound CH2 with molar mass 168 gmo?
The molecular formula of the compound CH2 with a molar mass of 168 g/mol is C8H16 since the molar mass of carbon is approximately 12 g/mol and the molar mass of hydrogen is approximately 1 g/mol. This is calculated by multiplying the subscripts in CH2 by their respective atomic masses and then calculating the total molar mass.
How do you calculate the grams of an element in a specific amount of a compound?
To calculate the grams of an element in a compound, you need to find the molar mass of the element and the compound. Then, use the formula: (mass of element/molar mass of compound) x molar mass of element. This will give you the grams of the element in the compound.
Why do you include water of crystallisation calculating molar mass?
You ca calculate the molar mass for an anhydrous compound or for the hydrated forms; it is your choice and depends on the available reagent.
How do you find the percent of oxygen by mass in a compound?
To find the percent of oxygen by mass in a compound, you need to know the molar mass of the compound and the molar mass of oxygen. Divide the molar mass of oxygen by the molar mass of the compound and multiply by 100 to get the percentage.
What is the percentage composition of molar mass in the given compound?
The percentage composition of molar mass in a compound is the percentage of each element's mass contribution to the total molar mass of the compound.
What is the molar mass of the nonelectrolyte compound if a 4.305 g sample of it is dissolved in 105 g of water?
To find the molar mass of the nonelectrolyte compound, we need to use the formula: Molar mass (mass of compound / moles of compound) First, we need to find the moles of the compound by using the formula: moles mass / molar mass Given that the mass of the compound is 4.305 g and it is dissolved in 105 g of water, we can calculate the moles of the compound. Next, we can find the molar mass of the compound by rearranging the formula: Molar mass mass / moles By plugging in the values, we can calculate the molar mass of the nonelectrolyte compound.
Compound made from 63.50 silver 8.25 nitrogen and 28.25 oxygen with a total molar mass 169.91g?
The compound is silver nitrate (AgNO3). By calculating the molar mass of the compound, which is 169.91 g/mol, we can determine the molecular formula. The molar mass of silver is 107.87 g/mol, nitrogen is 14.01 g/mol, and oxygen is 16.00 g/mol. The molar mass of silver nitrate matches the given value.
Does the molar mass of a compound change depending on the weight of the compound?
Molar mass depend on the ,mass,type and number of atoms in molecules of compound.
What is the molecular formula of the compound CH2 with molar mass 168 gmo?
The molecular formula of the compound CH2 with a molar mass of 168 g/mol is C8H16 since the molar mass of carbon is approximately 12 g/mol and the molar mass of hydrogen is approximately 1 g/mol. This is calculated by multiplying the subscripts in CH2 by their respective atomic masses and then calculating the total molar mass.
How do you calculate the grams of an element in a specific amount of a compound?
To calculate the grams of an element in a compound, you need to find the molar mass of the element and the compound. Then, use the formula: (mass of element/molar mass of compound) x molar mass of element. This will give you the grams of the element in the compound.
What is the molecular formula of the compound ch2 with molar mass equals 168 gmol?
c12h24
Which statement shows how to correctly convert from the mass of a compound in grams to the amount of that compound in moles?
To convert from the mass of a compound in grams to the amount of that compound in moles, you need to divide the mass of the compound in grams by its molar mass (which is found on the periodic table). This will give you the number of moles of the compound. The formula to use is: moles = mass (g) / molar mass.
How do you find theoretical percent of water?
To find the theoretical percent of water in a compound, you need to determine the molar mass of the compound and the molar mass of water. Then, divide the molar mass of water by the molar mass of the compound and multiply by 100 to get the percentage.
What is the relationship between the molar mass and the composition of a compound?
The molar mass of a compound is directly related to its composition. The molar mass is the sum of the atomic masses of all the elements in the compound. The composition of a compound refers to the types and amounts of elements present in it. Therefore, the molar mass provides information about the composition of a compound by indicating the relative amounts of each element present.
