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
Mass of Cr2O3 =151.99 g/mol
We know atomic mass of oxygen =16g
Mass of oxygen in chromium oxide =(16×3/151.99 )×60.8
=19.20g
Percentage of Chromium= (41.6/41.6+19.20)×100%
=68.42%
Percentage of oxygen = (19.2/41.6+19.2)× 100%
=31.57%
Element | Percentage of element | atomic mass | moles of atom | mole ratio |
Chromium | 68.42 | 52 | 1.315 | 1 |
Oxygen | 31.57 | 16 | 1.973 | 1.5 |
Now rounding off to simplest whole no ratio
Chromium =2
Oxygen= 3
Therefore empirical formula = Cr2O3
If 41.6g of chromium is fully reacted with oxygen to produce 60.8g of chromium oxide, what...
If 0.586 grams of lead reacted with oxygen and 0.677 grams of the lead oxide is formed, what is the empirical formula of the compound?
Chromium reacts with oxygen to produce chromium oxide. 4Cr(s)+3O2(g)→2Cr2O3(s) Calculate the mass of Cr2O3 that can be produced if the reaction of 58.5 g of chromium and sufficient oxygen has a 78.0 % yield.
(16 points) If 1.000 g of chromium metal produces 1.461 g of chromium oxide, what is the empirical formula of the product?
A 3.556g sample of a pure aluminum oxide decomposes under heat to produce 1.674g of oxygen in addition to pure aluminum metal. What is the empirical formula of the aluminum oxide?
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
Copper(I) oxide will react with oxygen gas to produce copper(II) oxide. If 95.3 g of copper(I) oxide is reacted, how many grams of oxygen will be needed?
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 _____
1. When 2.50 g of copper metal reacts with molecular oxygen, the copper oxide product of the reaction has a mass of 2.81 g. What is the empirical formula of the copper oxide product 2. When 10.8 g of silver was reacted with sulfur. 12.4 grams of product was produced there was only one product). What is the empirical formula of the product? 3. Lysine is a compound composed of carbon, hydrogen, nitrogen and oxygen. When 1.50 g of lysine is burned,...
A0.500-g sample of tin foil reacted with oxygen to give 0.635 g of product. Calculate the empirical formula of the tin oxide. Refer to Example Exercise 1 Record your numbers to 3 significant figures. Do not use exponential notation or subscripts in your answers. a) The mass of oxygen used in the reaction is b) The number of moles of tin is moles and the number of moles of oxygen is moles. c) Using their ratio of number of moles,...
A 1.000-g sample of lead shot reacted with oxygen to give 1.077 g of product. Fill-in the blanks, to finally determine the empirical formula of the lead oxide. Refer to Example Exercise 1 Record your numbers to 3 significant figures. Do not use exponential notation or subscripts in your answers. a) The mass of oxygen used in the reaction is b) The number of moles of lead is moles and the number of moles of oxygen is moles. c) Using...