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Molar mass of CuSO4= 63.5 + 32 +4 x 16=63.5 + 96= 159.5g
Wiki User
∙ 14y ago
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.
Wiki User
∙ 12y ago249.72 g/mol
Anonymous
Wiki User
∙ 13y ago250 or 249.612g/mol
Wiki User
∙ 12y ago159.6086 g/mol
Wiki User
∙ 13y ago249.7 g/mol
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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 weight in grams of 3.36 1023 molecules of copper sulfate?
What is the weight in grams of 3.36 × 1023 molecules of copper sulfate (CuSO4)?
How much CuSO4.5H2O is required to prepare 100mL of a 0.050 M aqueous stock solution?
Approximately 0.31 grams of CuSO4.5H2O is needed to prepare 100mL of a 0.050 M solution. The molar mass of CuSO4.5H2O is 249.68 g/mol. First, calculate the moles of CuSO4 needed (0.1 L x 0.050 mol/L = 0.005 mol). Then convert moles to grams using the molar mass.
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.
How much copper is present in 100g of copper sulphate?
You can answer this question using a molar mass calculation for CuSO4. 63.55 g Cu + 32.06 g S + 4(16.00 g O) = 159.55 g CuSO4 In 159.55 g CuSO4, there are 63.55 g Cu. Use this as a conversion factor. 100 g CuSO4 x 63.55 g Cu = 39.8 g Cu .................... 159.55 g CuSO4
What is the formula mass of CuSO4 x 5H2O?
The relative formula mass of CuSO4.5H2O is worked out from the following masses:Cu = 63.55S = 32.06O x 9 = 16 x 9 = 144H x 10 = 1 x 10 = 10Adding these up, we get a relative formula mass of 249.61, often rounded up to 250. This means that one mole of CuSO4.5H2O weighs 249.61g.
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
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 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 weight in grams of 3.36 1023 molecules of copper sulfate?
What is the weight in grams of 3.36 × 1023 molecules of copper sulfate (CuSO4)?
What mass of na2s2o3 5h2o is needed to prepare 500.00 ml of 0.1000 m na2s2o3?
To calculate the mass needed, you first need to determine the molar mass of Na2S2O3•5H2O. Then use the formula: mass = molarity (M) x volume (L) x molar mass (g/mol). Substitute the values to find the mass of Na2S2O3•5H2O needed.
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
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
How much CuSO4.5H2O is required to prepare 100mL of a 0.050 M aqueous stock solution?
Approximately 0.31 grams of CuSO4.5H2O is needed to prepare 100mL of a 0.050 M solution. The molar mass of CuSO4.5H2O is 249.68 g/mol. First, calculate the moles of CuSO4 needed (0.1 L x 0.050 mol/L = 0.005 mol). Then convert moles to grams using the molar mass.
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.
How many moles are in 44.78 g of cupric sulfate?
To find the number of moles in 44.78 g of cupric sulfate (CuSO4), first calculate the molar mass of CuSO4. The molar mass of CuSO4 is 159.61 g/mol. Next, divide the given mass by the molar mass to find the number of moles. Therefore, 44.78 g ÷ 159.61 g/mol = 0.281 moles of CuSO4.
What is the molar mass of K3PO4?
The molar mass of K3PO4 (potassium phosphate) is calculated by adding the atomic masses of all the elements present in the compound. Molar mass of K3PO4 = (3 x molar mass of K) + (1 x molar mass of P) + (4 x molar mass of O) = (3 x 39.10 g/mol) + (1 x 30.97 g/mol) + (4 x 16.00 g/mol) = 212.27 g/mol.
