In the decomposition of 1.00 g of aluminum sulfide, how many grams of each elemnt should be produced? You need to write your own balanced equation here. Aluminum sulfide= aluminum+ sulfur

0.36g of Al

0.64g of S

Explanation:

Let us write a balanced equation for the decomposition of aluminium sulfide Al2S3. This is shown below:

Al2S3 —> 2Al + 3S

Molar Mass of Al2S3 = (2x27) + (3x32) = 54 + 96 = 150g/mol

Molar Mass of Al = 27g/mol

Mass of Al from the balanced equation = 2 x 27 = 54g

Molar Mass of S = 32g/mol

Mass of S from the balanced equation = 3 x 32 = 96g

Now we can obtain the mass of Al and S produce as follows:

For Al:

From the equation,

150g of Al2S3 produced 54g of Al.

Therefore, 1g of Al2S3 will produce = 54/150 = 0.36g of Al.

For S:

From the equation,

150g of Al2S3 produced 96g of S.

Therefore, 1g of Al2S3 will produce = 96/150 = 0.64g of S

it's all four options.