0
6.02 x 1023
Wiki User
∙ 10y ago
Add your answer:
Earn +20 pts
How many formula units are there in 98.2g of LiCl?
The formula mass of the ionic compound lithium chloride, LiCl is 6.9 + 35.5 = 42.4.Amount of LiCl = 98.2/42.4 = 2.32molThere are 2.32 moles of formula unit in a 98.2g pure sample of LiCl.To get the numerical number, multiply the quantity in moles by the Avogadro's constant.
How many types of molecules with different masses exist in a sample of chlorine gas if the same exists entirely as diatomic molecules?
3
How many loaned pairs of electrons does LiCl have?
LiCl does not have any loaned pairs of electrons. In LiCl, lithium donates one electron to chlorine to form an ionic bond, leading to a full outer shell for both elements.
How are atoms related to molecules in a sample of a compound?
Atoms are the building blocks of molecules. Molecules are formed when two or more atoms chemically combine through bonds. A sample of a compound is made up of these molecules, which in turn are made up of individual atoms.
How many moles are there in 160g of bromine molecules?
Amount of Br2 = mass of sample / molar mass = 160 / 2(79.9) = 1.00mol
How many molecules of LiCl are in a 127.17g sample?
To calculate the number of molecules of LiCl in a 127.17g sample, you first need to determine the number of moles of LiCl in the sample using the molar mass of LiCl (6.94g/mol for Li and 35.45g/mol for Cl). Then, you can use Avogadro's number (6.022 x 10^23) to convert moles to molecules.
How many molecules are in LiCi are in a 127.17 g sample?
To determine the number of molecules in a sample of LiCl, we need to first calculate the number of moles using the molar mass of LiCl (42.39 g/mol). Next, we use Avogadro's number (6.022 x 10^23 molecules/mol) to convert moles to molecules. In this case, there are approximately (127.17 \text{ g} / 42.39 \text{ g/mol} \approx 3 \text{ moles} \times 6.022 \times 10^{23} \text{ molecules/mole} ≈ 1.8 \times 10^{24}) molecules of LiCl in 127.17 g.
How many formula units of LiCl are in 127.17 g sample?
127.17 g LiCl x 1 mol/42.4 g x 6.02x10^23 Form.Units/moles = 1.81x10^24 Formula Units.
How many formula units of LiCl are in a 127.17 g sample?
127.17 g LiCl x 1 mol/42.4 g x 6.02x10^23 Form.Units/moles = 1.81x10^24 Formula Units.
How many molecules are there in 9.34 grams of water?
Assuming the question refers to LiCl (Lithium chloride) which has a molecular weight 42.39. Avogadro's constant states there are 6.022 141 79x1023 molecules per mole 9.34 g LiCl is 9.34/42.39 mole (0.220 mole) LiCl The number of molecules is therefore 6.022 141 79x1023x 0.220 =1.326x1023 molecules
How many formula units are there in 98.2g of LiCl?
The formula mass of the ionic compound lithium chloride, LiCl is 6.9 + 35.5 = 42.4.Amount of LiCl = 98.2/42.4 = 2.32molThere are 2.32 moles of formula unit in a 98.2g pure sample of LiCl.To get the numerical number, multiply the quantity in moles by the Avogadro's constant.
How many molecules are contained in a 6.30g sample of dimethylmercury?
To find the number of molecules in a 6.30g sample of dimethylmercury, you need to know the molar mass of dimethylmercury (the molecular formula is C2H6Hg) and Avogadro's number. First, calculate the number of moles in the sample by dividing the mass by the molar mass. Then, use Avogadro's number to convert moles to molecules by multiplying by 6.022 x 10^23.
How many molecules are contained in a 7.85-g sample of dimethylmercury?
To determine the number of molecules in a sample, we need to know the molar mass of dimethylmercury (C2H6Hg). The molar mass of dimethylmercury is approximately 230.62 g/mol. Using this molar mass, we can calculate that there are approximately 2.23 x 10^22 molecules in a 7.85-g sample of dimethylmercury.
How many molecules of H2(g) are there in a 21.25 gram sample?
To calculate the number of molecules, you first need to determine the number of moles of H2 in the 21.25 gram sample using the molar mass of H2 (2 grams/mol). Then, use Avogadro's number (6.022 x 10^23 molecules/mol) to convert moles to molecules.
How many molecules of water does a 50g sample of H2O have?
A 50g sample of H2O contains approximately 2.78 x 10^24 molecules of water. This is calculated by first converting the mass to moles, then using Avogadro's number to determine the number of molecules present in that many moles of water.
How many molecules are present in the C3H4 sample?
There are Avogadro's number of molecules present in one mole of any substance. For C3H4, the molecules in one mole would be equal to Avogadro's number multiplied by 3 (for 3 carbon atoms) plus 4 (for 4 hydrogen atoms), which equals 3 * 6.022 x 10^23 + 4 * 6.022 x 10^23 = 26.056 x 10^23 molecules.
How many molecules are contained in a 5.20-g sample of dimethylmercury?
To calculate the number of molecules in a 5.20-g sample of dimethylmercury, you first need to determine the molar mass of dimethylmercury (Me2Hg). Then, you can use Avogadro's number (6.022 x 10^23 molecules/mol) to convert the mass to moles and then to molecules.
