A strip of iron weighing 0.95g is placed in the flask and allowed to react with the sulfur. If the weight of the new compound is 77g, determine:
(Fe = 55.85g/mol and S = 32.06g/mol)
a. The mass of sulfur reacted = _______________
b. The mass percent Fe and S based on the experiment
%Fe =
%S =
c. The empirical formula of the compound.
A strip of iron weighing 0.95g is placed in the flask and allowed to react with...
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
When 1.1338 g of an organic iron compound containing Fe, C, H, and O was burned in 02, 2.1207 g of CO2 and 0.60692 g of H2O were produced. In a separate experiment to determine the mass percent of iron, 0.6461 g of the compound yielded 0.1460 g of Fe,O3. What is the empirical formula of the compound?
-- 0 02 -.UJU U CILJI UUUU. 26. A 3.78 g sample of iron metal is reacted completely with sulfur to produce 5.95 g of iron sulfide. Determine the empirical formula and enpirical formula mass of this compound.
When 1.3213 g of an organic iron compound containing Fe, C, H, and O was burned in O2, 2.4714 g of CO2 and 0.70728 g of H2O were produced. In a separate experiment to determine the mass percent of iron, 0.6161 g of the compound yielded 0.1392 g of Fe2O3. What is the empirical formula of the compound?
When 1.4083 g of an organic iron compound containing Fe, C, H, and O was burned in O2, 2.6341 g of CO2 and 0.75385 g of H2O were produced. In a separate experiment to determine the mass percent of iron, 0.4231 g of the compound yielded 0.09559 g of Fe2O3. What is the empirical formula of the compound?
. Iron pyrite, commonly known as fool’s gold is 46.5% Fe and 53.5% S. a) If the empirical formula and the molecular formula are the same what is the molecular formula of the compound? b) If the crystal contains 4.85 g of iron then how much sulfur is in the crystal?
1.53 g of aluminum metal is placed in a Erlenmeyer flask with 1.5 M sulfuric acid. The hydrogen gas produced from the reaction is collected over water as seen in the diagram below. The aluminum is allowed to react with the sulfuric acid until it stops reacting. There is still some unreacted aluminum left in the reaction flask. The gas in the collection flask is brought to the same atmospheric pressure as the surroundings, 765.25 torr and a temperature of...
1. When 4.912 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 15.41 grams of CO2 and 6.311 grams of H2O were produced.In a separate experiment, the molar mass of the compound was found to be 28.05 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon.Enter the elements in the order presented in the question.empirical formula =molecular formula =2. When 6.848 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 21.49 grams of CO2 and 8.799 grams of H2O were produced.In a separate experiment, the molar mass...
Question 1 (1 marks) Tron (II) sulfide can react with carbonic acid, H2CO3, according to the reaction shown. 2 FeS (s) + H2CO3 (aq) + 2 FeO (s) + 1/n (CH2O)n (aq) + 2 S (s) NO a) Calculate the mass (g) of iron (II) oxide produced when 10.20 g iron (II) sulfide and 1.450 mol carbonic acid are reacted. The reaction results in a 87.5 % yield of product formed. b) If the carbon containing product has a molar...
A flask is charged with 0.124 mol of A and allowed to react to form B according to the reaction A(g) B(g). The following data are obtained for A as the reaction proceeds: The average rate of disappearance of A between 20.0 s and 40.0 s is ________ mol/s Select one: A. 1.4 × 10–3 B. 7.1 × 10–3 C. 8.5 × 10–4 D. 1.7 × 10–3 E. 590 Time (S) 0.0 10.0 20.0 30.0 40.0 Moles of A 0.124...