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What mass of anhydrous copper 2 sulfate can be obtained by heating 125g of cuper 2 sulfate pentahydrate?
To find the mass of anhydrous copper(II) sulfate obtained: Calculate the molar mass of each compound: CuSO4·5H2O (pentahydrate) and CuSO4 (anhydrous). Use the molar ratio between CuSO4 and CuSO4·5H2O to find the amount of anhydrous CuSO4. Convert the amount to mass using the molar mass of CuSO4. The mass of anhydrous CuSO4 will be less than the initial 125g due to the loss of water upon heating.
Suppose 2.3754g of copper-II sulfate pentahydrate is heated to drive off the water of crystallization Calculate what mass of anhydrous salt will remain?
The gram formula unit mass of copper (II) sulfate pentahydrate is 249.68. The gram formula unit mass of water is 18.015. Therefore, the mass of water of crystallization present in 50.0 g of copper (II) sulfate pentahydrate is: 50[5(18.015)/249.68] or 18.0 g, to the justified number of significant digits. (Note that the prefix penta- means five)
How many grams of copper(II) sulfate pentahydrate would you need to measure in order to have 10.0 grams of anhydrous copper (II) sulfate?
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.
Does hydrated copper sulphate increase the mass?
When hydrated copper sulfate is heated, it loses water molecules and forms anhydrous copper sulfate, which has a lower mass due to the removal of water. So, the mass would decrease upon heating hydrated copper sulfate.
Mass in grams if the molar mass of sodium sulfate is 141.98 gramsmoles?
To calculate the mass in grams of sodium sulfate, we need to know the number of moles. Once we have the number of moles, we can multiply it by the molar mass to find the mass in grams. For example, if we have 2 moles of sodium sulfate, the mass would be 2 moles * 141.98 grams/mole = 283.96 grams.
How many moles is 44.78g of cupric sulfate?
To find the number of moles, you need to divide the given mass (44.78g) by the molar mass of cupric sulfate. The molar mass of cupric sulfate (CuSO4) is approximately 159.61 g/mol. Therefore, 44.78g of cupric sulfate is approximately 0.28 moles.
What is the molar mass for anhydrous(without water) barium sulfate?
The molar mass for anhydrous barium sulfate (BaSO4) is 233.43 g/mol
Yonas has 44.78 g of cupric sulfate How many moles does he have?
To find the number of moles of cupric sulfate, we need to divide the given mass by its molar mass. The molar mass of cupric sulfate (CuSO4) is approximately 159.61 g/mol. 44.78 g / 159.61 g/mol ≈ 0.281 moles Therefore, Yonas has approximately 0.281 moles of cupric sulfate.
If 13.0g of MgSO47H2O is thoroughly heated what mass of anhydrous magnesium sulfate will remain?
8.79 grams of magnesium sulfate will remain.
What mass of anhydrous copper 2 sulfate can be obtained by heating 125g of cuper 2 sulfate pentahydrate?
To find the mass of anhydrous copper(II) sulfate obtained: Calculate the molar mass of each compound: CuSO4·5H2O (pentahydrate) and CuSO4 (anhydrous). Use the molar ratio between CuSO4 and CuSO4·5H2O to find the amount of anhydrous CuSO4. Convert the amount to mass using the molar mass of CuSO4. The mass of anhydrous CuSO4 will be less than the initial 125g due to the loss of water upon heating.
How many moles are in 44.78 g of cupric sulfate?
CuSO4 (cupric sulfate) has a molecular weight of 159.602g/mol Cu=63.546 S =32.06 O = 15.999 x 4 =63.996 Add the atomic weights of the elements in cupric sulfate. This is 159.602 grams/mol. Now divide the number of grams( 44.78) by the molecular weight of cupric sulfate (159.602). 44.78 g CuSO4/159.602 g/mol CuSO4= .2805 mol(moles) of cupric sulfate. The answer is 0.2805
How many moles are present in 480g of anhydrous magnesium sulfate?
First we calculate the formula mass of the compound magnesium sulfate.Formula mass of MgSO4 = 24.3 + 32.1 + 4(16.0) = 120.4 Amount of MgSO4 in a 480g pure sample = 480/120.4 = 3.99mol There is approximately 4 moles of the compound present in a 480g sample.
Yonas has 44.78 g of cupric sulfate. How many moles does he have?
Cupric sulfate is CuSO4 which has a molar mass of 159.6g/mol. Thus 44.78 g x 1 mol/159.6 g = 0.2806 moles (to 4 significant figures).
Suppose 2.3754g of copper-II sulfate pentahydrate is heated to drive off the water of crystallization Calculate what mass of anhydrous salt will remain?
The gram formula unit mass of copper (II) sulfate pentahydrate is 249.68. The gram formula unit mass of water is 18.015. Therefore, the mass of water of crystallization present in 50.0 g of copper (II) sulfate pentahydrate is: 50[5(18.015)/249.68] or 18.0 g, to the justified number of significant digits. (Note that the prefix penta- means five)
How many grams of copper(II) sulfate pentahydrate would you need to measure in order to have 10.0 grams of anhydrous copper (II) sulfate?
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.
If add water to a copper sulfate crystal will it get larger?
Copper(II) sulfate can fom 3 hydrates; the molar mass increase from the anhydrous salt to heptahydrate.
When calculating the number of moles of solid Na2SO4 the factor used is?
The molar mass of anhydrous sodium sulfate is 142,04.
