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 (CuSO4)?
The weight/weight of CuSO4 in the saturated solution is 20%. This means that for every 100 grams of the solution, 20 grams are CuSO4.
Well, darling, to produce 29.8g of water, you'd need to heat 249.9g of copper sulfate pentahydrate. When you heat it, the water molecules will be driven off, leaving you with just the copper sulfate. Just make sure to wear your safety goggles, we don't need any accidents in the name of science!
Copper (II) sulphur pentahyrdrate has the molecular formula of CuSO4x5H20, The molecular compound is composed of copper (Cu), sulphur (S), oxygen (O), and hydrogen (H). Its molecular weight is 249.7 grams per mole.
The formula mass of copper (II) sulfate, CuSO4, is calculated by adding the atomic masses of copper (Cu), sulfur (S), and four oxygen atoms (O) in the compound. The atomic masses are approximately: Cu = 63.5, S = 32.1, O = 16. The formula mass of CuSO4 is 63.5 + 32.1 + 4(16) = 159.5 grams/mole.
What is the weight in grams of 3.36 × 1023 molecules of copper sulfate (CuSO4)?
What is the weight in grams of 3.36 × 1023 molecules of copper sulfate (CuSO4)?
Copper(II) sulfate contain 398,1339 g copper in 1 kg CuSO4.
The weight/weight of CuSO4 in the saturated solution is 20%. This means that for every 100 grams of the solution, 20 grams are CuSO4.
Well, darling, to produce 29.8g of water, you'd need to heat 249.9g of copper sulfate pentahydrate. When you heat it, the water molecules will be driven off, leaving you with just the copper sulfate. Just make sure to wear your safety goggles, we don't need any accidents in the name of science!
No, 1750 mL of water is not enough to dissolve 4.6 g of copper sulfate (CuSO4) as the solubility of CuSO4 in water is about 203 g/L at room temperature. You would need more water to dissolve 4.6 g of CuSO4 completely.
Copper (II) sulphur pentahyrdrate has the molecular formula of CuSO4x5H20, The molecular compound is composed of copper (Cu), sulphur (S), oxygen (O), and hydrogen (H). Its molecular weight is 249.7 grams per mole.
The molecular weight of CuSO4 (copper (II) sulfate) is approximately 159.61 grams per mole. This value is calculated by adding the atomic weights of copper (Cu), sulfur (S), and four oxygen (O) atoms in one mole of the compound.
29.8g H2O = 1.66 mol H2O Molar Mass CuSO4 * 5H2O = 249.6 g mol CuSO4 * 5H2O --> 5 mol H2O 249.6 g CuSO4 * 5H2O/1 mol CuSO4 * 5H2O Times * 1mol CuSO4 * 5H2O/5mol H2O Times* 1.66 mol H2O = 82.6 g CuSO4 * 5H2O
The formula mass of copper (II) sulfate, CuSO4, is calculated by adding the atomic masses of copper (Cu), sulfur (S), and four oxygen atoms (O) in the compound. The atomic masses are approximately: Cu = 63.5, S = 32.1, O = 16. The formula mass of CuSO4 is 63.5 + 32.1 + 4(16) = 159.5 grams/mole.
To calculate this, you would need to consider the molar masses of copper(II) sulfate pentahydrate and anhydrous copper(II) sulfate. Copper(II) sulfate pentahydrate has a molar mass that includes water molecules, so you need to determine the molar mass difference between the two compounds. Using this information, you can calculate the amount of copper(II) sulfate pentahydrate needed to obtain 10.0 grams of anhydrous copper(II) sulfate.
At 60°C, about 31.6 g of copper (II) sulfate will dissolve in 100 g of water. This means that about 3.4 g of copper (II) sulfate will not dissolve and will form a saturated solution.