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Oh, dude, the formula mass of CuSO4 x 5H2O is calculated by adding up the atomic masses of copper (Cu), sulfur (S), oxygen (O), and hydrogen (H) in the compound. So, let's see... Cu has a mass of around 63.5, S is about 32.1, O is roughly 16, and H is like 1. So, when you add all that up, you get the formula mass. Easy peasy, right?
What else can I help you with?
What is the formula for hydrated copper II sulfate?
Copper sulfatepentahydrate is a solid at 20 degrees Celsius has a density of 2.28g/cm3 (cubed)... and its' chemical symbol is CuSO4-5H2O
What mass of na2s2o3 5h2o is needed to prepare 500.00 ml of 0.1000 m na2s2o3?
Mol.Wt =248.17Molarity =( Wt/ Mol.Wt ) /No:of litres of solution0.1 =( Wt / 248.17) / 0.5Wt =0.1 *0.5*248.17Wt = 12.4085g in 500ml of solution.
What is the equation for copper II chloride hexahydrate?
Cu(NO3)2 x 5H2O is the chemical formula for copper II nitrate pentahydrate.
What is the formula for cupric sulfate hydrate?
The formula for cupric sulfate hydrate is CuSO4 · xH2O, where x represents the number of water molecules associated with each copper sulfate molecule.
What is the percent by mass of sulfur in CuSO4?
The molar mass of CuSO4 is 159.61 g/mol. The molar mass of sulfur (S) is 32.06 g/mol. To find the percent by mass of sulfur in CuSO4, we calculate: (32.06 g/mol / 159.61 g/mol) x 100% = 20.07%. Therefore, sulfur makes up about 20.07% of the mass of CuSO4.
What is the molar mass of CuSo4 x 5H2O?
The molar mass of CuSO4 x 5H2O (copper (II) sulfate pentahydrate) is calculated by adding the molar mass of CuSO4 (159.61 g/mol) to five times the molar mass of water (5 * 18.02 g/mol). Therefore, the molar mass of CuSO4 x 5H2O is 249.72 g/mol.
What is the formula for hydrated copper II sulfate?
Copper sulfatepentahydrate is a solid at 20 degrees Celsius has a density of 2.28g/cm3 (cubed)... and its' chemical symbol is CuSO4-5H2O
What is the percentage of water CuSO4 5H2O?
First of all, it's CuSO4*5H2O (notice the capital "O" in the first part of the formula). The compound is called copper(II) sulfate pentahydrate, and if we wish to find the percent by mass of water, we need to find the molar mass of the hydrate first. Cu = 63.55 g/molS = 32.07 g/molO x 4 = 16.00 g/mol x 4 = 64.00 g/molH2O x 5 = 18.02 g/mol x 5 = 90.10 g/molNow add them all together and you get a molar mass of 249.72 g/molOf that 249.72 grams, 90.10 grams is water, so to find the percentage by mass that is water, simply divide 90.10 g by 249.72 g and multiply the result by 100%:90.10 g / 249.72 g x 100% = 36.08% water
How to find Number of oxygen atoms in 10.037 grams of CuSO4.5H2O?
Molar mass of CuSO4.5H2O = 250 No. of moles = 10.037 / 250 = 0.040 No. of molecules = 0.040 * 6.02 * 10^23 = 2.417 x 10^22 1 molecule of CuSO4.5H2O gives 9 O atoms --> No. of O atoms = 2.417 x 10^22 x 9 = 2.175 x 10^23
What is the value of x if mass of CuSO4.xH2O and mass of CuSO4 is given after heated?
The value of x can be determined by comparing the masses of CuSO4.xH2O and CuSO4 before and after heating. By calculating the difference in mass, the value of x can be obtained based on the loss of water molecules during the heating process.
What mass of na2s2o3 5h2o is needed to prepare 500.00 ml of 0.1000 m na2s2o3?
Mol.Wt =248.17Molarity =( Wt/ Mol.Wt ) /No:of litres of solution0.1 =( Wt / 248.17) / 0.5Wt =0.1 *0.5*248.17Wt = 12.4085g in 500ml of solution.
What is the equation for copper II chloride hexahydrate?
Cu(NO3)2 x 5H2O is the chemical formula for copper II nitrate pentahydrate.
How many grams would 3.36 1023 molecules of copper (II) sulfate (CuSO4) weigh?
To calculate the weight of 3.36 x 10^23 molecules of CuSO4, you would first find the molar mass of CuSO4 (159.61 g/mol). Then, you'd use this molar mass to convert the number of molecules to grams using the formula: grams = (molecules x molar mass) / Avogadro's number. This would give you the weight of 3.36 x 10^23 molecules of CuSO4.
What is the formula for cupric sulfate hydrate?
The formula for cupric sulfate hydrate is CuSO4 · xH2O, where x represents the number of water molecules associated with each copper sulfate molecule.
What is the percent by mass of sulfur in CuSO4?
The molar mass of CuSO4 is 159.61 g/mol. The molar mass of sulfur (S) is 32.06 g/mol. To find the percent by mass of sulfur in CuSO4, we calculate: (32.06 g/mol / 159.61 g/mol) x 100% = 20.07%. Therefore, sulfur makes up about 20.07% of the mass of CuSO4.
How much CuSO4.5H2O is required to prepare 100mL of a 0.050 M aqueous stock solution?
RMM of CuSo4 . 5H2O = 160 + 5x18 = 250 g How much contain gram in 100 mL of 0.050 M CuSO4 solution is - Solution: = 0.050 x 100/1000 x 250 = 0.050x4 (100)/ 16 = 1.25 g
Find the percentage of water to the nearest tenth in crystal of CuSo4 x 5H2O?
The atomic mass of CuSO4 is 159.61 g/mol, and that of 5 H2O is 90.08 g/mol. To find the percentage of water, we calculate (90.08 g/mol / (90.08 g/mol + 159.61 g/mol)) * 100, which is approximately 36.1%. So, the crystal contains around 36.1% water to the nearest tenth.
