What mass of iron is needed to react with sulfur in order to produce 96 grams of iron (|||) sulfide according to the following equation?
2fe+3s—> fe2s3

51.57 g.

Explanation:

n = mas/molar mass = (96.0 g)/(207.9 g/mol) = 0.46 mol.

Using cross multiplication we can get the no. of moles of Fe that isn eeded to produce 0.46 mol of Fe₂S₃:

2.0 moles of Fe produces → 1.0 mol of Fe₂S₃.

??? moles of Fe produces → 0.46 mol of Fe₂S₃.

∴ The no. of moles of Fe needed = (2.0 mol)(0.46 mol)/(1.0 mol) = 0.92 mol.

mass = no. of moles x molar mass = (0.92 mol)(55.845 g/mol) = 51.57 g.

the temperature of the gas, in k, not celsius.

b. accuracy of the data matters alot more than its number of digits, organization or amount of detail. quantitative observation is more accepted than the qualitative observation.