It depends on the substance you are measuring and is specific to that substance. More information is needed
The answer is 125,65 g.
The balanced chemical equation for the formation of iron oxide is: 4 Fe + 3 O2 -> 2 Fe2O3. From the equation, we see that 4 moles of iron are required to produce 2 moles of iron oxide. Therefore, with 8.00 mol of iron, we can produce 4.00 mol of iron oxide. To find the mass of iron oxide produced, we multiply the moles of Fe2O3 by its molar mass, which is approximately 159.7 g/mol. This gives us 4.00 mol x 159.7 g/mol = 638.8 grams of iron oxide produced.
To find the mass of 1.40 mol of iron (III) sulfate (Fe2(SO4)3), you need to calculate the molar mass of the compound. Iron (III) sulfate has a molar mass of approximately 399.9 g/mol. Therefore, the mass of 1.40 mol of iron (III) sulfate would be 1.40 mol x 399.9 g/mol = 559.86 grams.
The number of moles is 4.
To calculate the amount of iron in Fe2S3, first find the molar mass of Fe2S3: Iron (Fe) has a molar mass of 55.85 g/mol and sulfur (S) has a molar mass of 32.06 g/mol. So, the molar mass of Fe2S3 is 2(55.85) + 3(32.06) = 222.92 g/mol. Next, divide the molar mass of iron by the molar mass of Fe2S3 and multiply by the given mass of Fe2S3 to find the grams of iron: (2 * 55.85 g/mol / 222.92 g/mol) * 34 g = 8.53 g of iron in 34 g of Fe2S3.
To calculate the number of iron atoms in 0.0178 mol of iron, you can use Avogadro's number, which is 6.022 x 10^23 atoms/mol. Number of iron atoms = 0.0178 mol x 6.022 x 10^23 atoms/mol = 1.07 x 10^22 atoms.
The answer is 125,65 g.
The balanced chemical equation for the formation of iron oxide is: 4 Fe + 3 O2 -> 2 Fe2O3. From the equation, we see that 4 moles of iron are required to produce 2 moles of iron oxide. Therefore, with 8.00 mol of iron, we can produce 4.00 mol of iron oxide. To find the mass of iron oxide produced, we multiply the moles of Fe2O3 by its molar mass, which is approximately 159.7 g/mol. This gives us 4.00 mol x 159.7 g/mol = 638.8 grams of iron oxide produced.
Five iron atoms have a mass of 1.3155 x 10-22 grams.
To find the number of moles of iron (Fe) in 223.2 g, you can use the formula: moles = mass (g) / molar mass (g/mol). The molar mass of iron is approximately 55.85 g/mol. Thus, moles of iron = 223.2 g / 55.85 g/mol ≈ 3.99 moles.
To find the mass of 1.40 mol of iron (III) sulfate (Fe2(SO4)3), you need to calculate the molar mass of the compound. Iron (III) sulfate has a molar mass of approximately 399.9 g/mol. Therefore, the mass of 1.40 mol of iron (III) sulfate would be 1.40 mol x 399.9 g/mol = 559.86 grams.
Iron is approximately 2.7 times heavier than aluminum. This is due to the difference in their atomic weights - iron has an atomic weight of 55.85 g/mol, while aluminum has an atomic weight of 26.98 g/mol.
The number of moles is 4.
To calculate the amount of iron in Fe2S3, first find the molar mass of Fe2S3: Iron (Fe) has a molar mass of 55.85 g/mol and sulfur (S) has a molar mass of 32.06 g/mol. So, the molar mass of Fe2S3 is 2(55.85) + 3(32.06) = 222.92 g/mol. Next, divide the molar mass of iron by the molar mass of Fe2S3 and multiply by the given mass of Fe2S3 to find the grams of iron: (2 * 55.85 g/mol / 222.92 g/mol) * 34 g = 8.53 g of iron in 34 g of Fe2S3.
Number of particles=number of moles x avogadro constant = 25.9 x 6.02 x 1023
7.2
To find the number of moles in 233.2 g of iron (Fe), you need to divide the given mass by the molar mass of iron, which is approximately 55.85 g/mol. So, 233.2 g ÷ 55.85 g/mol ≈ 4.17 moles of iron.