You react 4.40 grams of iron filings (elemental iron) with excess sulfur in an experiment. You find that the mass of your iron sulfide product is 5.67 g. The empirical formula of that product is Fe3S2
Ir2S3
FeS
Fe2S
IrS
Sol.
As Mass of iron , Fe = 4.40 g
Molar Mass of Fe = 55.845 g/mol
So , Moles of Fe = 4.40 g / 55.845 g/mol = 0.0788 mol
Also , Mass of sulphur , S
= Mass of iron sulfide product - Mass of Iron
= 5.67 g - 4.40 g
= 1.27 g
Molar Mass of S = 32.065 g/mol
Moles of S = 1.27 g / 32.065 g/mol = 0.0396 mol
Divide both the moles of Fe and S by the smallest number
Moles of Fe = 0.0788 / 0.0396 = 2
Moles of S = 0.0396 / 0.0396 = 1
Therefore ,
Emperical Formula of iron sufide is Fe2S
You react 4.40 grams of iron filings (elemental iron) with excess sulfur in an experiment. You...
6. What mass of iron (Fe) is needed to react with 16.0 grams of sulfur (Ss)? 8 Fe +S8 ->8 FeS
write clearly c. If 1.164 g of iron filings react with chlorine gas to give 3.384 g of iron chloride, what is the empirical formula of the compound? 2 marks
5. A 1.000-g sample of iron metal reacted with sulfur powder to give 1.574 g of prod Calculate the empirical formula of the iron sulfide.6. A 1.000-g sample of iron metal reacted with sulfur powder to give 1.861 g of product Calculate the empirical formula of the iron sulfide.
A 2.41g sample of iron powder (Fe) reacted with 1.405 g of sulfur(S). Calculate the empirical formula of the iron sulfide product.
If 150.0 grams of Fe2O3 react in excess carbon monoxide, what mass of iron will be produced? If in an experiment only 87.9 grams of Fe were recovered, what is the percent yield of this reaction
For the following reaction, 26.5 grams of sulfur dioxide are allowed to react with 6.34 grams of water sulfur dioxide(g)+ water(l) sulfurous acid (H2SO3)(g) What is the maximum mass of sulfurous acid (H2SO3) that can be formed? grams What is the FORMULA for the limiting reagent? What mass of the excess reagent remains after the reaction is complete? grams Submit Answer Retry Entire Group 6 more group attempts remaining
Sulfur and oxygen react to produce sulfur trioxide. In a particular experiment, 7.9 grams of SO3 are produced by the reaction of 9.0 grams of O2 with 10.0 grams of S. What is the % yield of SO3 in this experiment? S (s) + O2 (g) → SO3 (g) (not balanced)
For the following reaction, 14.7 grams of sulfur are allowed to react with 19.3 grams of carbon monoxide . sulfur(s) + carbon monoxide(g) → sulfur dioxide(g) + carbon(s) What is the maximum amount of sulfur dioxide that can be formed? | grams What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? grams
7) Calculate the mass in grams of FE2S3 (iron III sulfide) that can be produced with 375 grams of Fe (iron) based on the following equation: (1.5 point) Fe2S3(s) 3S(s) 2Fe(s) Show all your calculations above, then circle your best answer d) 415.8 g Fe2S c) 623.7 g Fe2S3 b) 698 g Fe2S3 a) 207.9 g Fe2S3
For the following reaction, 16.9 grams of sulfur are allowed to react with 21.1 grams of carbon monoxide. sulfur ($)+ carbon monoxide (8) —>sulfur dioxide (g) + carbon (5) What is the maximum amount of sulfur dioxide that can be formed? grams What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? grams