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Which is the greatest mass of SO2 that can produced from 15.0 mol 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.
What is the mass in grams of a single formula unit of copper(I) sulfide Cu2S?
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
What is the mass of a formula unit of cuprous sulfide?
The mass of a formula unit of cuprous sulfide (Cu2S) is 159.152 g/mol.
What is the mass of this sulfur (Density of sulfur 2.07 gcm3.)?
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.
What is the percent mass of sulfur in sulfur dioxide?
69
How many moles is 22 grams of Cu2S?
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
How many kilograms of copper sulfide could be formed from reaction of 0.90mol of copper with excess sulfur?
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!
Which is the greatest mass of SO2 that can produced from 15.0 mol 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.
What is the mass in grams of a single formula unit of copper(I) sulfide Cu2S?
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
Why sulphur increase its weight after dry and burnt?
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.
What is the exact percent composition of copper in pure chalcocite?
Chalcocite's chemical formula is Cu2S, meaning it consists of 80% copper and 20% sulfur by mass.
What is the mass of a formula unit of cuprous sulfide?
The mass of a formula unit of cuprous sulfide (Cu2S) is 159.152 g/mol.
What is the mass of this sulfur (Density of sulfur 2.07 gcm3.)?
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.
What is the percent by mass of sulfur in sulfur dioxide?
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%.
What is the mass number sulfur?
Sulfur is a non metallic element. Mass number of it is 32.
What is the the mass number of sulfur?
Atomic number for sulfur: 16
What percent of metal does g of metal combines with g of oxygen?
The percentage of metal that combines with oxygen can be calculated using the formula: (mass of metal / total mass) * 100%. For example, if 2g of metal combines with 4g of oxygen to form an oxide, the percentage of metal that combines with oxygen is (2g / (2g + 4g)) * 100% = 33.3%.
