{ [ 8.0(g) / 63.55(g/molCu) ] / 2(2Cu per S) } * 32(g/molS) = 2.0 g Sulfur.
All dimensions are in 'brackets ( ) directly following the number.
To find the maximum mass of SO2 produced from 15.0 mol of Cu2S, first determine the molar ratio between Cu2S and SO2. The balanced chemical equation shows that 4 mol of SO2 is produced for every 1 mol of Cu2S consumed. Thus, you would produce 60.0 mol of SO2 from 15.0 mol of Cu2S. Finally, convert the moles of SO2 to grams using the molar mass of SO2 to find the mass.
Cu(I) sulfide has the formula Cu2S. Thus the mass in grams of a single formula unit is 63.5 x 2 = 127 for two coppers32.1 x 1 = 32.1 for one STotal = 159.1
The mass of a formula unit of cuprous sulfide (Cu2S) is 159.152 g/mol.
To find the mass of the sulfur, we need the volume of the sulfur sample. If we have the volume, we can multiply it by the density of sulfur to calculate the mass. Without the volume of the sulfur sample, we cannot determine its mass.
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First you need to write a balanced chemical equation: 2Cu + S >> Cu2S Then you use dimensional analysis to solve and convert to kilograms: 0.90 mol Cu x 1 mol Cu2S/2 mol Cu x 159.166g Cu2S x 1kgCu2S/10^3g Cu2S= 7.2 x 10^-2 kg Cu2S Hope this helps!
One definition of a mole is the sum of the average atomic weights (mass) of a compound. In this case 2 Copper + 1 Sulfur = (2 * 63.55) + (1 * 32.07) = 159.17 grams per mole. So 22 g / 159.17 g/mole = 0.14 mole of Cu2S
To find the maximum mass of SO2 produced from 15.0 mol of Cu2S, first determine the molar ratio between Cu2S and SO2. The balanced chemical equation shows that 4 mol of SO2 is produced for every 1 mol of Cu2S consumed. Thus, you would produce 60.0 mol of SO2 from 15.0 mol of Cu2S. Finally, convert the moles of SO2 to grams using the molar mass of SO2 to find the mass.
Cu(I) sulfide has the formula Cu2S. Thus the mass in grams of a single formula unit is 63.5 x 2 = 127 for two coppers32.1 x 1 = 32.1 for one STotal = 159.1
When sulfur is burned, it combines with oxygen from the air to form sulfur dioxide (SO2) gas. This reaction results in an increase in weight as sulfur gains mass from the oxygen atoms it combines with during the reaction. Additionally, any impurities or contaminants present in the sulfur may contribute to the increase in weight after it is burned.
Chalcocite's chemical formula is Cu2S, meaning it consists of 80% copper and 20% sulfur by mass.
The mass of a formula unit of cuprous sulfide (Cu2S) is 159.152 g/mol.
To find the mass of the sulfur, we need the volume of the sulfur sample. If we have the volume, we can multiply it by the density of sulfur to calculate the mass. Without the volume of the sulfur sample, we cannot determine its mass.
The molar mass of sulfur dioxide (SO2) is 64.06 g/mol. The molar mass of sulfur is 32.06 g/mol. Calculate the mass percent of sulfur in SO2 using the formula (mass of sulfur / mass of SO2) x 100%. This gives a mass percent of sulfur in SO2 as 50%.
Sulfur is a non metallic element. Mass number of it is 32.
Atomic number for sulfur: 16
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