Barium is a more active metal than aluminium. In fact, the lower elements in the activity series gains electrons from the higher elements, which are also called as displacement reactions. The final products of this reaction would be barium sulfide and aluminium metal.
The reaction isȘ
BaO + H2O = Ba(OH)2
3BaS + 2Al is most likely the product.
The product is Ba(OH)2.
Yes, called aluminum sulfide, Al2S3
2Al + 3S -> Al2S3
S2Ur5 NO this is wrong! There isn't even an element that is Ur wow! The answer is Al2S3
The answer i got is 12.33 grams of Al2S3. Below i will try to show the steps i used: n=moles m=mass (grams) M= molecular weight (from periodic table) 2Al + 3S --> Al2S3 nAl= m/M = 9/13 = 0.692307 moles of Al nS= m/M = 8/16 = 0.5 moles of S Limiting Reagent: 1.5 moles of S required for every mole of Al (3:2 ratio) This means that there should be about 1.04 moles of S to completely use up all the Al. Since there is less than this amount of S present (only 0.5 moles), S is the limiting reagent and should be used in the mole calculation of the product Amount of product: 0.5 moles S x (1 mol Al2S3/ 3 mol S) = 0.16666 moles of Al2S3 nAl2S3 = m/M Molecular weight of Al2S3 = (2 x 13) + (3 x 16) = 74 0.16666 moles Al2S3 = m/74 m = 74 x 0.16666 = 12.33 grams of Al2S3 Therefore, 12.33 grams of Al2S3 is formed in this reaction ( hopefully this is right :P )
Yes
2Al + 3S ==> Al2S3
Yes, called aluminum sulfide, Al2S3
2Al + 3S -> Al2S3
2Al + 3S -> Al2S3
2Al+3S--->Al2S3
The chemical equation is:2 Al + 3 S = Al2S3
100/150.158 is 0.666 moles
Aluminium sulfide is not soluble in water; Al2S3 is easily hydrolyzed.
510 g Al2S3 is equal to 3,396 moles.
S2Ur5 NO this is wrong! There isn't even an element that is Ur wow! The answer is Al2S3
The answer i got is 12.33 grams of Al2S3. Below i will try to show the steps i used: n=moles m=mass (grams) M= molecular weight (from periodic table) 2Al + 3S --> Al2S3 nAl= m/M = 9/13 = 0.692307 moles of Al nS= m/M = 8/16 = 0.5 moles of S Limiting Reagent: 1.5 moles of S required for every mole of Al (3:2 ratio) This means that there should be about 1.04 moles of S to completely use up all the Al. Since there is less than this amount of S present (only 0.5 moles), S is the limiting reagent and should be used in the mole calculation of the product Amount of product: 0.5 moles S x (1 mol Al2S3/ 3 mol S) = 0.16666 moles of Al2S3 nAl2S3 = m/M Molecular weight of Al2S3 = (2 x 13) + (3 x 16) = 74 0.16666 moles Al2S3 = m/74 m = 74 x 0.16666 = 12.33 grams of Al2S3 Therefore, 12.33 grams of Al2S3 is formed in this reaction ( hopefully this is right :P )
Yes