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The mass of 6.02 x 10^23 atoms of calcium (Ca) is approximately 40.08 grams. This Atomic Mass value is based on the molar mass of calcium, which is 40.08 g/mol.
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What is the mass in grams of 6.022 x 1023 N atoms of mass 14.01 amu?
The molar mass of any element is its atomic weight (amu) in grams, and 1 mol of any element is 6.022 x 1023 atoms. Therefore, the mass in grams of 6.022 x 1023 atoms of N = 14.01g N.
Most calcium atoms have an atomic number of 20 and a mass number of 40 but some calcium atoms have a mass number of 48 What word could you use to describe these two kinds of calcium atoms?
Isotopes. Calcium atoms with a mass number of 40 represent the most common isotope, while those with a mass number of 48 are a less common, but still natural, isotopic form of calcium.
How many atoms are in 173 grams of calcium?
Hi!So there's this formula triangle which I can't do on here but which, put into an equation is: Mass (g) = RAM (Relative atomic mass of the element) x Number of Moles.Now, you know the amount of calcium there is (173g), and, by checking a periodic table and finding Ca and the big number next to it, you know Calcium's RAM (40.08). From this, you can find the number of moles (and from there, you can find the number of atoms, I think) because..... Number of Moles = Mass (173g) / RAM (40.08)Which gives you ~4.32 moles.There are6.02 x 1023 (Avocado's number or something :D) atoms in a mole, and as youhave ~4.32 moles, 4.32 x6.02 x 1023 = 2.60064x1024This might not be the easiest way, but it's the only one I could think of! Hope it helps!
How many atoms are in 159g of calcium?
To find the number of atoms in 159g of calcium, you need to first calculate the number of moles of calcium present using the molar mass of calcium. The molar mass of calcium is approximately 40 g/mol. Then, you can use Avogadro's number (6.022 x 10^23 atoms/mol) to convert moles of calcium to atoms. Calculate the number of moles of calcium in 159g using the formula: moles = mass (g) / molar mass (g/mol). Finally, multiply the number of moles by Avogadro's number to determine the number of atoms in 159g of calcium.
How many atoms are in 149 g of calcium?
To calculate the number of atoms in 149 g of calcium, you first need to convert the grams to moles using the molar mass of calcium. The molar mass of Calcium is 40.08 g/mol. Then, you can use Avogadro's number (6.022 x 10^23 atoms/mol) to find the number of atoms in the moles of calcium.
How many atoms are in 125 grams of Calcium?
Well, Ca has an atomic mass of 40, so one mole of Ca (6.022x1023 atoms) equals 40g.To get 5kg of Ca, you would times the 40g (one mole) by 125.5kg of Ca has 125x(6.022x1023), or602200000000000000000000 atoms.
How many atoms are in 115 grams of Calcium?
Avogadro's Number, 6.022 x 1023 gives the number of atoms in one mole. Calcium has an average atomic weight of 40.08 gmol-1 So one mole weighs 40.08 grams. 115 grams of Calcium will have (6.022 x 1023 / 40.08)*115 = 1.73 x 1024 atoms.
How many atoms are in 139 g of calcium?
Amount of Ca = 139/40.1 = 3.47mol 1 mol of Ca contains 6.02 x 1023 atoms (avogadro constant). 3.47mol of Ca thus contains 3.47 x 6.02 x 1023 = 2.09 x 1024 atoms
How many atoms are in 1.0g of hydrogen atoms each mass 1.0amu?
6.023 x 1023 atoms
How many atoms are present in 7.92g of calcium fluoride?
Calculate the number of moles of calcium fluoride by dividing the mass by its molar mass. The molar mass of calcium fluoride (CaF2) is 78.08 g/mol. Then, multiply the number of moles by Avogadro's number (6.022 x 10^23) to find the number of atoms present in 7.92g of calcium fluoride.
How many atoms are in sucrose table sugar?
1 mole has 12.01 grams and has 6.022 x 1023 atoms. There are 6 carbon atoms in a glucose molecule so that times six would give you a total of 72.06 grams out of the 180.156 (molar mass for glucose). Carbon makes up about 40 percent of the total glucose mass so the final answer would be it would be around 2.4088 x 1023 atoms of carbon in one gram. Times that by 4 and you'll get 9.6352 x 1023 atoms of carbon in four gram of glucose.
What is the mass in grams of 6.022 x 1023 N atoms of mass 14.01 amu?
The molar mass of any element is its atomic weight (amu) in grams, and 1 mol of any element is 6.022 x 1023 atoms. Therefore, the mass in grams of 6.022 x 1023 atoms of N = 14.01g N.
What is the mass of 8.90 x 1023 lead atoms?
8.90 X 1023 lead atoms (1 mole Pb/6.022 X 1023)(207.2 grams/1 mole Pb) = 306 grams of lead =============
How many atoms in 1 gram of calcium?
To find the number of atoms in 1 gram of calcium, you can use Avogadro's number and the molar mass of calcium. The molar mass of calcium is approximately 40.08 grams per mole. Therefore, 1 gram of calcium is about 0.0249 moles (1 g / 40.08 g/mol). Multiplying this by Avogadro's number (approximately (6.022 \times 10^{23}) atoms/mole) gives roughly (1.50 \times 10^{22}) atoms in 1 gram of calcium.
How do you find the mass of a sample of 1.72 x 1023 atoms of potassium?
1 mole K atoms = 39.0983g K (atomic weight in grams)1 mole K atoms = 6.022 x 1023 atoms K (Avogadro's number)Convert known atoms to moles.1.72 x 1023 atoms K x (1mol K/6.022 x 1023 atoms K) = 0.286mol KConvert moles to mass in grams.0.286mol K x (39.0983g K/1mol K) = 11.2g K
How many atoms are in 181 g of calcium?
To find the number of atoms in 181 g of calcium, first calculate the number of moles of calcium using its molar mass (40.08 g/mol). This comes to 4.5 moles. Next, use Avogadro's number (6.022 x 10^23 atoms/mol) to convert moles to atoms. Therefore, there are approximately 2.7 x 10^24 atoms in 181 g of calcium.
How many calcium atoms are in 35.6 g of calcium?
To find the number of calcium atoms in 35.6 grams of calcium, you first need to calculate the number of moles of calcium. The molar mass of calcium (Ca) is approximately 40.08 g/mol. Thus, the number of moles in 35.6 g is 35.6 g ÷ 40.08 g/mol ≈ 0.887 moles. Since one mole contains Avogadro's number of atoms (approximately (6.022 \times 10^{23}) atoms/mole), the total number of calcium atoms is about (0.887 \times 6.022 \times 10^{23} \approx 5.34 \times 10^{23}) atoms.
