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kirza4 [7]
2 years ago
11

Molecule contains carbon, hydrogen and sulfur atoms. When a sample of 0.535g of this compound is burnt in oxygen, 1.119 g of CO2

and 0.229 gof H2O and 0.407g of SO2are obtained.
Calculate its empirical formula.
Chemistry
1 answer:
OLga [1]2 years ago
4 0

Answer:

The empirical formula is, C4H4S

Explanation:

Number of moles of carbon = 1.119 g/ 44g/mol = 0.025 moles

Mass of Carbon= 0.025 moles × 12 g/ mole = 0.3 g

Number of moles of hydrogen = 0.229/18g/mol × 2 = 0.025 moles

Mass of hydrogen = 0.025 moles × 1 = 0.025 g

Number of moles of sulphur = 0.407g/ 64 g/mol = 0.0064 moles

Mass of sulphur= 0.0064 moles ×32 = 0.2 g

Now we obtain the mole ratios by dividing through by the lowest ratio.

C- 0.025 moles/ 0.0064 moles, H- 0.025 moles/ 0.0064 moles, S- 0.0064 moles/0.0064 moles

C4H4S

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The following compound has been found effective in treating pain and inflammation (J. Med Chem. 2007, 4222). Which sequence corr
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<h3><u>Full Question:</u></h3>

The following compound has been found effective in treating pain and inflammation (J. Med. Chem. 2007, 4222). Which sequence correctly ranks each carbonyl group in order of increasing reactivity toward nucleophilic addition?

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C) 3 < 1 < 2

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The rate of nucleophilic attack of carbonyl compounds is 2<3 <1.

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<h3><u>Explanation. </u></h3>

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7 0
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Bromine has two isotopes, Br79 and Br81. The isotopes occur in a 50:50 (1:1) ratio. Given that the mass spectrum of bromine cont
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Answer:

There will be 3 peaks.

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We are told that Bromine has two isotopes namely 79Br and 81Br in a 1 : 1 ratio (50 : 50).

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79Br¯ 81Br+ = 160

81Br¯ 81Br+ = 162

7 0
3 years ago
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