Al2(SO4)3 [anhydrous] = 342,15 Al2(SO4)3 [octadecahydrate] = 648,41
In aluminum sulfate, the molar mass of aluminum is 27 g/mol. Calculate the amount of aluminum in 5.60 g of aluminum sulfate using the molar ratio between aluminum and aluminum sulfate (1:1). Therefore, there are 5.60 grams of aluminum in 5.60 grams of aluminum sulfate.
The molar mass of aluminum sulfate (Al2(SO4)3) is approximately 342 grams per mole.
To find the amount of aluminum needed to produce aluminum sulfate, you need to consider the molar mass of aluminum sulfate and the ratio of aluminum in the compound. First, calculate the molar mass of aluminum sulfate (Al2(SO4)3). Then, find the ratio of aluminum in the compound (2 moles of Al in 1 mole of Al2(SO4)3). Finally, use this information to calculate the grams of aluminum needed to produce 25.0 grams of aluminum sulfate.
To find the number of moles of sulfur in 2.55g of aluminum sulfate, you need to first calculate the molar mass of aluminum sulfate (Al2(SO4)3), which is 342.15 g/mol. Sulfur accounts for 3 moles in one mole of aluminum sulfate, so you can calculate the number of moles by dividing the given mass (2.55g) by the molar mass of aluminum sulfate.
To convert grams of aluminum sulfate to moles, you first need to determine the molar mass of aluminum sulfate (Al2(SO4)3), which is approximately 342.15 g/mol. Then, divide the given mass by the molar mass to obtain the number of moles. In this case, 6.7 grams of aluminum sulfate is approximately 0.02 moles.
342.15
In aluminum sulfate, the molar mass of aluminum is 27 g/mol. Calculate the amount of aluminum in 5.60 g of aluminum sulfate using the molar ratio between aluminum and aluminum sulfate (1:1). Therefore, there are 5.60 grams of aluminum in 5.60 grams of aluminum sulfate.
The molar mass of aluminum sulfate (Al2(SO4)3) is approximately 342 grams per mole.
To find the mass of 0.25 moles of aluminum sulfate, you need to know the molar mass of aluminum sulfate. The molar mass of aluminum sulfate (Al2(SO4)3) is approximately 342.15 g/mol. Therefore, the mass of 0.25 moles of aluminum sulfate would be around 85.54 grams.
The molar mass of aluminum sulfate, Al2(SO4)3, can be calculated by adding together the atomic masses of all the elements in the compound. Aluminum has a molar mass of 26.98 g/mol, sulfur has a molar mass of 32.06 g/mol, and oxygen has a molar mass of 16.00 g/mol. By calculating the total molar mass, the molar mass of aluminum sulfate is found to be approximately 342.14 g/mol.
To find the amount of aluminum needed to produce aluminum sulfate, you need to consider the molar mass of aluminum sulfate and the ratio of aluminum in the compound. First, calculate the molar mass of aluminum sulfate (Al2(SO4)3). Then, find the ratio of aluminum in the compound (2 moles of Al in 1 mole of Al2(SO4)3). Finally, use this information to calculate the grams of aluminum needed to produce 25.0 grams of aluminum sulfate.
To find the number of moles of sulfur in 2.55g of aluminum sulfate, you need to first calculate the molar mass of aluminum sulfate (Al2(SO4)3), which is 342.15 g/mol. Sulfur accounts for 3 moles in one mole of aluminum sulfate, so you can calculate the number of moles by dividing the given mass (2.55g) by the molar mass of aluminum sulfate.
To convert grams of aluminum sulfate to moles, you first need to determine the molar mass of aluminum sulfate (Al2(SO4)3), which is approximately 342.15 g/mol. Then, divide the given mass by the molar mass to obtain the number of moles. In this case, 6.7 grams of aluminum sulfate is approximately 0.02 moles.
The molar mass of aluminum sulfate is 342.15 g/mol. Therefore, the mass of 0.25 moles of aluminum sulfate would be 85.54 grams (0.25 moles x 342.15 g/mol).
The molar mass of ammonium sulfate is 132,14 g.
159.61 grams per mole.
What is the weight in grams of 3.36 × 1023 molecules of copper sulfate (CuSO4)?