The molar mass of copper is its atomic weight on the Periodic Table in g/mol, and is
63.5g/mol
We know that one mole of copper contains
6.022×10^23 atoms of copper
. First convert given mass to moles, and moles to atoms.
= 61.0 g Cu × (1 mol Cu / 63.5 g per mol) ×6.022 × 10 ^23 atom cu / 1 mol Cu) = 5.78× 10^23.
atoms.
61 g Cu 5.7 ×10^23 atoms of Cu.
To calculate the number of Cu atoms in 85 mol, you need to use Avogadro's number, which is approximately 6.022 x 10^23 atoms/mol. So, for 85 mol of Cu, the number of Cu atoms would be 85 mol x 6.022 x 10^23 atoms/mol = 5.12 x 10^25 Cu atoms.
To convert grams of Cu to atoms, first calculate the molar mass of Cu from the periodic table (63.55 g/mol). Next, divide the given mass (12.54 g) by the molar mass to get moles of Cu. Finally, use Avogadro's number (6.022 x 10^23 atoms/mol) to convert moles to atoms.
To find the number of atoms in 1.2 grams of copper, you need to first determine the molar mass of copper (Cu). The molar mass of copper is 63.55 g/mol. Next, calculate the number of moles in 1.2 grams of copper (1.2 g / 63.55 g/mol = 0.0189 mol). Finally, use Avogadro's number (6.022 x 10^23 atoms/mol) to convert moles to atoms: 0.0189 mol x 6.022 x 10^23 atoms/mol = approximately 1.14 x 10^22 atoms.
To find the mass of 1.20x10^28 atoms of copper (Cu), you need to first calculate the molar mass of copper (Cu), which is approximately 63.55 g/mol. Then, convert the number of atoms to moles by dividing by Avogadro's number (6.022 x 10^23 atoms/mol). Finally, convert moles to kilograms by multiplying by the molar mass and dividing by 1000 to get the mass in kilograms.
Divide that number of atoms by 6.02x10^23 atoms/mole
To calculate the number of atoms in 3.01 x 10²³ atoms of copper (Cu), you simply interpret the notation. The expression indicates that there are 3.01 times 10 raised to the power of 23 atoms, which is a way to express a large quantity, specifically Avogadro's number (approximately 6.022 x 10²³). Thus, 3.01 x 10²³ atoms of copper is approximately half of Avogadro's number, indicating that you have about half a mole of copper atoms.
14.0 g x 1 mole/187.56 g = 0.0746 moles0.0746 moles Cu(NO3)2 x 6 moles O/mole Cu(NO3)2 = 0.448 moles O atoms0.448 moles O atoms x 6.02x10^23 atoms/mole = 2.70x10^23 atoms of oxygen
To determine the number of Cu atoms in the piece of sterling silver jewelry, you would first need to convert the weight of the jewelry to moles using the molar mass of silver. Then, since sterling silver is typically 92.5% silver and 7.5% copper by weight, you can calculate the number of moles of copper present. Finally, use Avogadro's number to convert from moles to atoms.
There are 2 nitrogen atoms in 1 molecule of copper(II) nitrate (Cu(NO3)2). To find the number of nitrogen atoms in 10.2 g of Cu(NO3)2, you first need to calculate the number of moles of Cu(NO3)2 in 10.2 g, then use the mole ratio to find the number of nitrogen atoms. The molar mass of Cu(NO3)2 is 187.56 g/mol.
To find the weight of 4.6 x 10^25 atoms of copper, you can start by calculating the molar mass of copper, which is approximately 63.55 g/mol. Next, convert the number of atoms to moles by dividing by Avogadro's number (6.022 x 10^23). Finally, multiply the number of moles by the molar mass to find the weight in grams.
The oxidation number of Cu in Cu2S (copper sulfide) is +1. This is because the overall charge of the compound is 0 and there are two Cu atoms each with an oxidation state of +1.
Cu(NO3)2 has 9 atoms 1 Cu atom 2 N atoms 6 O atoms