Chemistry, 09.10.2021 01:10 dschallipp
For each of the reactions, calculate the mass (in grams) of the product formed when 15.00 g of the underlined reactant completely reacts. Assume that there is more than enough of the other reactant.
2K(s)+Cl2(g)βββββββ2KCl(s)
Express your answer using four significant figures.
2K(s)+Br2(l)βββββββ2KBr(s)
Express your answer using four significant figures.
4Cr(s)+3O2(g)βββββββ2Cr2O3(s)
Express your answer using four significant figures.
2Sr(s)βββββ+O2(g)β2SrO(s)
Express your answer using four significant figures.
Answers: 1
Chemistry, 22.06.2019 11:50
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Chemistry, 22.06.2019 20:20
Nitric acid can be formed in two steps from the atmospheric gases nitrogen and oxygen, plus hydrogen prepared by reforming natural gas. in the first step, nitrogen and hydrogen react to form ammonia: (g) (g) (g) in the second step, ammonia and oxygen react to form nitric acid and water: (g) (g) (g) (g) calculate the net change in enthalpy for the formation of one mole of nitric acid from nitrogen, hydrogen and oxygen from these reactions. round your answer to the nearest .
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Chemistry, 22.06.2019 22:30
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Chemistry, 23.06.2019 04:31
One student said that the investigation was not valid (a fair test). write a plan for the investigation that includes improvements to the method and apparatus
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For each of the reactions, calculate the mass (in grams) of the product formed when 15.00 g of the u...
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