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How many atoms would be found in 1.2 grams of copper?
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.
How many atoms are present in 3.14g of Cu?
3.14 g Cu = # atomsTake the known mass of copper multiply it by Avogadro number and divided by the atomic weight.Atomic weight of copper:63.5 g3.14 g Cu (6.02 × 1023 atoms) / (63.5 grams) = 2.98 × 1022 atoms of Copper
How do you convert 12.54 g of Cu to 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.
How many Cu atoms are in the 0.0159 mol sample?
The molar mass of copper is approximately 63.5 g. To find how many of these are in our sample we must divide.0.0159/63.5 = 2.5 x 10 ^ -4 = 0.00025 moles. Each mole contains the Avogadro number of atoms, i.e. 6.023 x 10 ^ 23, so in total we have 0.00025x 6.023 x 10 ^ 23 = 1.51 x 10 ^ 20 atoms approximately.
How many grams of Cu would be needed to react with 2.0 mol HNO3?
The balanced chemical equation for the reaction between copper (Cu) and nitric acid (HNO3) is Cu + 4HNO3 -> Cu(NO3)2 + 2NO2 + 2H2O. From the equation, it can be seen that 1 mol of Cu reacts with 4 mol of HNO3. Therefore, to react with 2.0 mol of HNO3, 0.5 mol of Cu is needed. The molar mass of Cu is approximately 63.5 g/mol, so 0.5 mol of Cu would be equivalent to 31.75 grams.
How many Cu atoms are present in 85mol?
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.
How many atoms are in 1 mole of Copper?
1 mol Cu Atoms (6.02x10^23 atoms)
Calculate the number of atoms in 61.0 g of Cu?
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.
How many atoms would be found in 1.2 grams of copper?
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.
How do you get moles Chemistry?
The mole in chemistry is also called the chemist's dozen and is defined as the amount of material containing 6.0221421 X10^23 particles(This number is called Avogadro's number) The value of mole is the number of particles in excactly 12 grams of c-12, so, if you have 12grams of c-12 , you will have 6.022x10^23 carbon atoms ,which is also a mol of C. For any other element a mol of that element is the Atomic Mass expressed as grams. 0.0265 g C find mol of C plan gC -> mol C 1 mol / 12.01 g C ( relationship; 1 mol C = 12.01 g C ) 0.0265 g C x 1 mol C / 12.01 g C = 2.21 x 10 ^-3 mol C to find atoms change to mol then times 6.022X10^23 3.10g Cu find Cu atoms plan g -> mol cu -> atoms Cu (3.10 g cu )x (1 mol Cu /63.55 g Cu ) ( 6.022 x 10^23 / 1 mol cu = 2.94 x 10^22 Cu atoms
How many atoms are present in 3.14g of Cu?
3.14 g Cu = # atomsTake the known mass of copper multiply it by Avogadro number and divided by the atomic weight.Atomic weight of copper:63.5 g3.14 g Cu (6.02 × 1023 atoms) / (63.5 grams) = 2.98 × 1022 atoms of Copper
How do you convert 12.54 g of Cu to 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.
How many atoms of copper Cu are in a pure copper coin weighing 12.0 g?
Answer: 1.14x10^23 atoms Cu (12.0g Cu/63.55amu(g) Cu) Then take (Ans x 6.022x10^23) = 1.13712038x10^23 atoms Cu. Then I simplified it to 3 sig figs. = 1.14x10^23 atoms Cu Never forget your units and substance!
How many Cu atoms are in the 0.0159 mol sample?
The molar mass of copper is approximately 63.5 g. To find how many of these are in our sample we must divide.0.0159/63.5 = 2.5 x 10 ^ -4 = 0.00025 moles. Each mole contains the Avogadro number of atoms, i.e. 6.023 x 10 ^ 23, so in total we have 0.00025x 6.023 x 10 ^ 23 = 1.51 x 10 ^ 20 atoms approximately.
How many atoms are in 2.6 mol Cu?
To find the number of atoms in 2.6 moles of copper (Cu), you can use Avogadro's number, which is approximately (6.022 \times 10^{23}) atoms per mole. Multiply the number of moles by Avogadro's number: (2.6 , \text{mol} \times 6.022 \times 10^{23} , \text{atoms/mol} \approx 1.57 \times 10^{24} , \text{atoms}). Thus, there are approximately (1.57 \times 10^{24}) atoms in 2.6 moles of copper.
How many atoms of phosphorus are in 8.90 mol of copperII phosphate?
To find the number of phosphorus atoms in 8.90 mol of copper(II) phosphate (Cu₃(PO₄)₂), we first identify that each formula unit contains 2 phosphorus (P) atoms. Thus, in 8.90 mol of copper(II) phosphate, the total number of phosphorus atoms is calculated as follows: 8.90 mol × 2 P/mol = 17.8 mol of phosphorus atoms. To convert moles to atoms, we multiply by Avogadro's number (approximately (6.022 \times 10^{23}) atoms/mol): 17.8 mol × (6.022 \times 10^{23}) atoms/mol ≈ (1.07 \times 10^{24}) phosphorus atoms.
How many grams of Cu would be needed to react with 2.0 mol HNO3?
The balanced chemical equation for the reaction between copper (Cu) and nitric acid (HNO3) is Cu + 4HNO3 -> Cu(NO3)2 + 2NO2 + 2H2O. From the equation, it can be seen that 1 mol of Cu reacts with 4 mol of HNO3. Therefore, to react with 2.0 mol of HNO3, 0.5 mol of Cu is needed. The molar mass of Cu is approximately 63.5 g/mol, so 0.5 mol of Cu would be equivalent to 31.75 grams.
