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 the empirical formula and molecular formula of phosphorus oxide given the molar mass is approximately 282 g/mol?
5)
we have mass of each elements as:
Co: 0.565 g
S: 1.027 g - 0.565 g = 0.462 g
Divide by molar mass to get number of moles of each:
Co: 0.565/58.93 = 9.588*10^-3
S: 0.462/32.07 = 1.441*10^-2
Divide by smallest:
Co: 9.588*10^-3/9.588*10^-3 = 1
S: 1.441*10^-2/9.588*10^-3 = 1.5
Multiply by 2 to get simplest whole number ratio:
Co: 1*2 = 2
S: 1.5*2 = 3
So empirical formula is:Co2S3
Answer: Co2S3
Only 1 question at a time please
5. A 0.565-8 sample of cobalt metal reacted with excess sulfur powder to give 1.027 g of cobalt sulfide
40.505-8 sample of cobalt metal reacted with excess sulfur powder to give 1.027 g of cobalt sulfide. Calculate the empirical formula of the product. D. 565. Cox Imal Co 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.
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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...
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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 1.000g sample of red phosphorus powder was burned in air and.reacted with oxygen gas to give 2.291g of phosphorus oxide. calculate the empirical formula andmolecular formula of phosphorus oxide give the molar mass is approximately 282g/mol?
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