What is the mass of 6.02 x10 23 atoms of carbon?

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What is the mass of 6.02 x10 23 atoms of carbon?

Example: Carbon (atomic mass = 12.01) – 1 mole of Carbon weighs 12.01 grams. This means that 6.022×1023 carbon atoms (or molecules) weights 12.01 grams.

What is the amount of carbon dioxide produced when 1 mole of carbon is burnt in air?

44 g
i) when 1 mole of carbon is burnt in 1 mole(32 g) of air(dioxygen) ,then according to chemical equation (1) 1mole(44 g) of carbon dioxide is produced.

What will be the mass of one mole of carbon atoms select the correct answer below 12 g 12 amu 6.022 1023 g 6.022 1023 amu?

The mole is the link between the micro world of atoms and molecules to the macro world of grams and kilograms. By definition, NA 12C atoms, i.e. Avogadro’s number, 6.022×1023 12C atoms has a mass of 12.00⋅g .

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What is the mass of 6.02 x10 23?

Therefore, the mass in grams of 6.02 x 1023 atoms of the element is x g. From the periodic table, the element with the molar mass of 83.80 g/mol is Kr.

How many moles of carbon dioxide is produced when 1 mole of carbon reacts with 16g of oxygen?

We can conclude from the equation when 1 mole of carbon burnt in 1 mole of dioxygen (molecular mass = 32), gives rise to 1 mole of carbon dioxide (molecular mass=44). Now according to the question only 16g of dioxygen is available for the reaction. Number of moles of Oxygen = \[\dfrac{16}{32}\]= 0.5 moles.

When 1 mole of glucose is bond amount of carbon dioxide produced will be?

And then the next question is what masses of carbon dioxide and water in grams are formed. Remember, for every one mole of glucose, we needed six moles of molecular oxygen and we produce six moles of carbon dioxide and we produce six moles of water.

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What is the mass of 6 moles of carbon-12?

12.0⋅g
It means that NA (Avogadro’s number =6.022×1023) 12C atoms have a mass of 12.0⋅g . You have specified 6.0⋅g . Thus 6.0⋅g12.0⋅g⋅mol−1 = 0.50⋅mol .

What is the mass of 1 mole of carbon *?

12 grams
The mass of one mole of carbon-12 atoms is 12 grams. A mole is a set number of particles, whether that is atoms or molecules.

What is the atomic weight of 1 mole of carbon?

If 1 mole of carbon is 6.022*10^23 atoms of carbon, but 1 mole of carbon is also equal to 12 grams, then which is the atomic weight of C? – Quora If 1 mole of carbon is 6.022*10^23 atoms of carbon, but 1 mole of carbon is also equal to 12 grams, then which is the atomic weight of C? Get Visual Assist 2021.3 today.

How many atoms are there in 3 moles of CO2?

So, 3 moles of CO2 contains (3 x 2 x 6.02 x 10*23) O atoms = 3.61 x 10*24 O atoms. Likewise, how many atoms are there in one mole of carbon? 1 mole of carbon. Exactly 12 grams of pure carbon-12 powder is known as one mole. The number of atoms of carbon-12 present in this one mole sample is 6.022 136 7 x 1023.

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What is the number of atoms in 12 grams of carbon 12?

1 mole of carbon. Exactly 12 grams of pure carbon-12 powder is known as one mole. The number of atoms of carbon-12 present in this one mole sample is 6.022 136 7 x 1023. This number is known as Avogadro’s number.

How many atoms are in a mole of an element?

Mole: the amount of a substance that contains 6.02 x 1023 respective particles of that substance Avogadro’s number: 6.02 x 1023 Molar Mass: the mass of one mole of an element CONVERSION FACTORS: 1 mole = 6.02 x 1023 atoms 1 mole = atomic mass (g)