To determine the number of atoms in 16g of oxygen gas, you first need to calculate the number of moles of oxygen using the molar mass of oxygen. Oxygen has a molar mass of 16g/mol. So, 16g of oxygen gas is equal to 1 mole of oxygen gas. One mole of oxygen gas contains approximately 6.022 x 10^23 atoms (Avogadro's number). Therefore, 16g of oxygen gas contains approximately 6.022 x 10^23 oxygen atoms.
If you know the density of oxygen and the molar mass of oxygen you can divide the two in order to find the molar volume of oxygen. (L/mol) Oxygen has a density of 1.429 g/L and a molar mass of 32.00 g/mol. (Just remember that the molar mass of oxygen, chemical formula of 0 2, comes straight from the Periodic Table.) So, divide: 1.429 g/L / 32.00 g/mol = 22.393 L/mol. The "g" unit cancells out and you're left with L/mol which is your molar mass. Compare that with 22.4 L/mol which is the accepted molar volume for an ideal gas, derived from the ideal gas law: pv=nRt. However, because most gases do not behave ideally there is a slight discrepancy.
The mass of 2.000 mol of oxygen atoms is 32.00 grams.
The molar mass of water(H2O)=18((1*2)+16)The no. of moles(n) of water in 18 g of water=mass/molar mass=18 g/ 18 g mol-1 =1 molThe no. of molecules of water in 18 of water=n*Avogadro no. =1 mol*6.022*1023 mol-1 =6.022*1023The no. of atoms of oxygen in one mole of water=1 molThe no. of atoms of oxygen in 6.022*1023mol of water= 6.022*1023
There are approximately 0.625 moles of oxygen gas in 40.0 grams. Since the formula for oxygen gas is O2, there are 0.625 moles x 2 = 1.25 moles of oxygen atoms. Therefore, there are approximately 1.25 x 6.022 x 10^23 = 7.53 x 10^23 oxygen atoms in 40.0 grams of oxygen gas.
To find the amount of oxygen used, we need to consider the difference in mass between sodium and sodium oxide. The mass increase is 16g (62g - 46g) which corresponds to the amount of oxygen used from the air. Therefore, 16g of oxygen from the air were used.
Iron(III) oxide is composed of one iron atom and three oxygen atoms. Therefore, if we have 44 grams of iron(III) oxide, we can calculate the mass of iron by subtracting the mass of oxygen. 44g - 16g (mass of oxygen) = 28g of iron is needed to combine with 16g of oxygen to form 44g of iron(III) oxide.
One mole of oxygen has a mass of 16 grams and contains 6.022 x 10^23 oxygen atoms. Therefore, 16 grams of oxygen will also contain 6.022 x 10^23 oxygen atoms.
1 mole of O has a mass of 16g and contains 6.022 x 10^23 atoms (Avogadro's number). Therefore, 16g of O would contain the same number of atoms, which is 6.022 x 10^23 atoms.
In 16g of O, there are approximately 3.02 x 10^23 atoms, as the atomic mass of oxygen is 16 g/mol. In 8g of S, there are approximately 6.02 x 10^23 atoms, as the atomic mass of sulfur is 32 g/mol.
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1mol O = 16.0g (rounded to 1 decimal place) 1mol O atoms = 6.022 x 1023 atoms 16g O x 1mol/16g = 1mol O 1mol O x 6.022 x 1023atoms/mol = 6.022 x 1023 atoms O
The mass of 2.000 mol of oxygen atoms is 32.00 grams.
The molar mass of water(H2O)=18((1*2)+16)The no. of moles(n) of water in 18 g of water=mass/molar mass=18 g/ 18 g mol-1 =1 molThe no. of molecules of water in 18 of water=n*Avogadro no. =1 mol*6.022*1023 mol-1 =6.022*1023The no. of atoms of oxygen in one mole of water=1 molThe no. of atoms of oxygen in 6.022*1023mol of water= 6.022*1023
The Avogadro number: 6,02214129(27)×1023.
To calculate the moles of carbon dioxide, we first need to determine the number of moles of oxygen in 16g. Using oxygen's molar mass of 16 g/mol, we find that there is 1 mole of oxygen in 16g. Since one mole of oxygen reacts with one mole of carbon dioxide in the balanced equation, there will also be 1 mole of carbon dioxide formed.
To calculate the number of atoms present in a given mass of a substance, we need to use the concept of molar mass and Avogadro's number. The molar mass of oxygen (O) is approximately 16 g/mol, and the molar mass of sulfur (S) is approximately 32 g/mol. For oxygen: 16g / 16 g/mol = 1 mol of O. 1 mol of O contains 6.022 x 10^23 atoms (Avogadro's number). Therefore, 16g of O contains 6.022 x 10^23 atoms. For sulfur: 8g / 32 g/mol = 0.25 mol of S. 0.25 mol of S contains 0.25 x 6.022 x 10^23 atoms = 1.5055 x 10^23 atoms. Therefore, there are approximately 6.022 x 10^23 atoms in 16g of oxygen and approximately 1.5055 x 10^23 atoms in 8g of sulfur.
Divide that number by Avogadro's number: 3.968x10(23) / 6.02x10(23) = 0.659mol Mg, which would be about 16g.
There are approximately 0.625 moles of oxygen gas in 40.0 grams. Since the formula for oxygen gas is O2, there are 0.625 moles x 2 = 1.25 moles of oxygen atoms. Therefore, there are approximately 1.25 x 6.022 x 10^23 = 7.53 x 10^23 oxygen atoms in 40.0 grams of oxygen gas.