40.505-8 sample of cobalt metal reacted with excess sulfur powder to give 1.027 g of cobalt...

Question

Question

40.505-8 sample of cobalt metal reacted with excess sulfur powder to give 1.027 g of cobalt sulfide. Calculate the empirical

Answer 1

Answer #1

58.93 32.1 mdles of Cobalt - 0.565, = 0.00959 moles mars of selber F1.027-0.565 +0.4629 moles of suffer= 0.462 0.0144 moles s

Answer 2

Similar Homework Help Questions

5. A 0.565-8 sample of cobalt metal reacted with excess sulfur powder to give 1.027 g of cobalt sulfide

5. A 0.565-8 sample of cobalt metal reacted with excess sulfur powder to give 1.027 g of cobalt sulfide Calculate the empirical formula of the product. 6. A 0.750-g sample of tin foil was heated in air and reacted with oxygen gas to give 0.953 g of tin oxide. Calculate the empirical formula of the product. 7. (optional) A 1.000-g sample of red phosphorus powder was burned in air and reacted with oxygen gas to give 2.291 g of phosphorus oxide. Calculate...
5-8 sample of cobalt metal reacted with excess salfiur powder to give 1.00 Calculate the empirical...

5-8 sample of cobalt metal reacted with excess salfiur powder to give 1.00 Calculate the empirical formula of the product olo. Imal Co 55-g sample of cobalt metal reacted with excess sulfur powder to give 1.027 - Calculate the empirical formula of the product.
A 1.000-g sample of iron metal reacted with sulfur powder to give 1.574 g of prod...

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.

1. A 0.750-g sample of tin metal reacts with 0.201 g of oxygen gas to form tin 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...
A 1.000-g sample of cobalt metal reacted with sulfur powder to give 1.548 g of product....

A 1.000-g sample of cobalt metal reacted with sulfur powder to give 1.548 g of product. Record your numbers to 3 significant figures. Do not use exponential notation or subscripts in your answers. a) The mass of sulfur used in the reaction is b) The number of moles of cobalt is moles and the number of moles of sulfur is moles. c) Using their ratio of number of moles, the empirical formula of the cobalt sulfide is Draw the Lewis...
A 0.500-g sample of chromium metal reacted with sulfur powder to give 0.963 g of product. a) The mass of sul...

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 _____

1.167-g sample of iron powder reacted with 0.680 g of sulfur powder to give iton oduct....

1.167-g sample of iron powder reacted with 0.680 g of sulfur powder to give iton oduct. Calculate the empirical formula of the iron sulfide.
A 2.41g sample of iron powder (Fe) reacted with 1.405 g of sulfur(S)

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.
A 43.29 gram sample of cobalt is heated in the presence of excess oxygen. A metal...

A 43.29 gram sample of cobalt is heated in the presence of excess oxygen. A metal oxide is formed with a mass of 60.92 g. Determine the empirical formula of the metal oxide.

A 50.63 gram sample of cobalt is heated in the presence of excess oxygen. A metal...

A 50.63 gram sample of cobalt is heated in the presence of excess oxygen. A metal oxide is formed with a mass of 71.25 g. Determine the empirical formula of the metal oxide Enter the elements in the order Co, O empirical formular