1.00 g of chromium metal produces 1.461 g of chromium oxide
weight of chromium in the sample = 1.00 g
mole of chromium = 1 g /51.9961 g/mol = 0.0192 mol
weight of O in the sample = 1.461-1.00 = 0.461 g
mole of O = 0.461 g/15.999 g/mol = 0.0288 mol
so the mole ratio of chromium and oxygen = 0.0288/0.0192 = 1.5
so in the oxide for 1 mol of chromium 1.5 moles of oxygen will be present
so the empirical formula of the oxide is Cr2O3
(16 points) If 1.000 g of chromium metal produces 1.461 g of chromium oxide, what is the empirical formula of the pr...
Show all work for the following problems answers only. partial credit will be given for work clearly shown. NO CREDIT will be given for .... . (10 points) If 1.000 g of chromium metal produces 1.461 g of chromium oxide, what is the empirical formula of the product?
Using the given formula of aluminum oxide, Al2O3, refer to the periodic table and predict the empirical formula for the oxide, B?O? A 0.500-g sample of chromium metal reacted with sulfur powder to give 0.963 g of product. a) The mass of sulfur that reacted is b) The empirical formula of the chromium sulfide is
If 41.6g of chromium is fully reacted with oxygen to produce 60.8g of chromium oxide, what is the empirical formula of the chromium oxide
1. A 0.750-g sample of tin metal reacts with 0.201 g of oxygen gas to form tin oxide. Calculate the empirical formula of the tin oxide. 2. A 0.565-g sample of cobalt metal reacts with excess sulfur to give 1.027 g of cobalt sulfide. Calculate the empirical formula of the product. 3. A 1.164-g sample of iron filings reacts with chlorine gas to give 3.384 g of iron chloride. Calculate the empirical formula of the product? 4. A 0.626-8 sample of copper oxide...
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 0.500-g sample of chromium metal reacted with sulfur powder to give 0.963 g of product. a) The mass of sulfur that reacted is _____ b) The empirical formula of the chromium sulfide is _____
20 Question (2 points) Chromium metal can be produced from the high temperature reaction of Cr2O3 [chromium(lII) oxide] with silicon or aluminum by each of the following reactions: 2Cr+ Al203 Cr203+2A 4Cr 3SIO2 2Cr203+3Si See Periodic Table (1 point) xFeedback Part 1 Calculate the number of grams of aluminum required to prepare 195.0 g of chromium metal by the first reaction. 169.7 See Hint (1 point) Part 2 X Calculate the number of grams of silicon required to prepare 195.0...
mass of magnesium metal?? Determine the empirical formula of Magnesium Oxide from following data. Show your calculations. Mass of Crucible and Cover + magnesium ribbon (before heating) 27.60 g Mass of crucible and Cover = 27.30 g Mass of magnesium metal = Mass of crucible and cover + magnesium oxide (after heating) = 27.80 Mass of combined oxide (after heating - before heating) =
14. A chemistry student determined the empirical formula for tungsten oxide (W Oy). To do so, he heated tungsten with oxygen in a crucible. The data that he recorded are shown below: Weight of crucible Weight of tungsten Weight of crucible and product 11.120 g 8.820 g 22.998 g a What is the percent composition by mass of tungsten oxide? D What is the empirical formula of tungsten oxide? (10 points)
A. Empirical Formula of Magnesium Oxide mass of crucible and cover + magnesium metal (before heating) 42.36 & 42.11 e 005 0 mass of crucible and cover 46.28 46.05. 011! 46.31 . 10 mass of magneſium metal mass of crucible and cover + magnesium oxide (after heating ) 42.49 & 0 bbb 10 0 mass of combined oxygen (after heating - before heating) w the calculation of the empirical formula for trial I (see Example Exercise 1).