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Elanso [62]
2 years ago
10

What is the empirical formula of a carbon-oxygen compound, given that a 95.2 g sample of the compound contains 40.8 g of carbon

and the rest oxygen?
Chemistry
1 answer:
algol [13]2 years ago
4 0

Answer:

95.2 - 40.8 = 54.4 g of oxygen

number of moles = mass (g)/ Mr

no. of moles of carbon = 40.8/12 = 3.4

no. of moles of oxygen = 3.4

divide both by smallest value which is 3.4 and you’ll get 1 mole of carbon and 1 mole of oxygen therefore the empirical formula is CO

Explanation:

hope this helps :)

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A stock solution of HNO3 is prepared and found to contain 13.5 M of HNO3. If 25.0 mL of the stock solution is diluted to a final
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Answer : The correct option is, (C) 0.675 M

Explanation :

Using neutralization law,

M_1V_1=M_2V_2

where,

M_1 = concentration of HNO_3 = 13.5 M

M_2 = concentration of diluted solution = ?

V_1 = volume of HNO_3 = 25.0 ml  = 0.0250 L

conversion used : (1 L = 1000 mL)

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Now put all the given values in the above law, we get the concentration of the diluted solution.

13.5M\times 0.0250L=M_2\times 0.500L

M_2=0.675M

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8 0
3 years ago
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Consequently, the <em>Noble gases ion</em> has a stable Valence electron configuration.

Read more:

brainly.com/question/5336231

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