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9966 [12]
3 years ago
13

A sample of a compound is analyzed and found to contain 0.420 g nitrogen, 0.480g oxygen, 0.540 g carbon and 0.135 g hydrogen. Wh

at is the empirical formula of the compound? a. C2H5NO b. CH3NO c. C3H9N2O2 d. C4HN3O4 e. C4H13N3O3
Chemistry
1 answer:
Crazy boy [7]3 years ago
7 0

Answer:

c. C3H9N2O2

Explanation:

The empirical formula of a compound is defined as the simplest whole number ratio of atoms present in a molecule. To solve this question we need to convert the mass of each atom to moles. With the moles we can find the ratio as follows:

<em>Moles N -Molar mass: 14.01g/mol-</em>

0.420g N * (1mol/14.01g) = 0.0300 moles N

<em>Moles O -Molar mass: 16g/mol-</em>

0.480g O * (1mol/16g) = 0.0300 moles O

<em>Moles C -Molar mass: 12.01g/mol-</em>

0.540g C * (1mol/12.01g) = 0.0450 moles C

<em>Moles H -Molar mass: 1.0g/mol-</em>

0.135g H * (1mol/1g) = 0.135moles H

Dividing in the moles of N (Lower number of moles) the ratio of atoms is:

N = 0.0300 moles N / 0.0300 moles N = 1

O = 0.0300 moles O / 0.0300 moles N = 1

C = 0.0450 moles C / 0.0300 moles N = 1.5

H = 0.135 moles H / 0.0300 moles N = 4.5

As the empirical formula requires whole numbers, multiplying each ratio twice:

N = 2, O = 2, C = 3 and H = 9

And the empirical formula is:

<h3>c. C3H9N2O2</h3>

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Sergeu [11.5K]

Answer: The correct option is heterogeneous mixture whose components are attracted differently to a magnet.

Explanation: There are two types of mixtures:

1) Homogeneous mixtures: In these mixtures, the particles are uniformly distributed throughout the mixture. These particles cannot be separated.

2) Heterogeneous Mixtures: These are the mixtures where the particles are visible separated and are not-uniformly distributed. These particles can be separated easily.

If magnet is used to separate the components of a mixture, the heterogeneous mixtures will only get separated.

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An amphoteric species is neither an acid nor a base. True or False
umka2103 [35]

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8 0
3 years ago
In the following reaction, how many grams of NaBr will react with 311 grams of Pb(NO3)2?
Mashutka [201]
Molar mass :

NaBr = 103 g/mol

Pb(NO3)2 = 331.20 g/mol

<span><span /><span>Balanced chemical equation :

</span></span>2 NaBr + 1 Pb(NO3)2 = 2 NaNO3 + 1 PbBr<span>2
</span><span>
2*103 g NaBr ------------> 1 * 331.20 g Pb(NO3)2
      g NaBr  -------------------> 311 g Pb(NO3)2

331.20  g  =   2*103*311

331.20 g = 64066

mass ( NaBr ) =  64066 / 331.20

mass ( naBr)  = 193,43 g of NaBr

hope this helps!.


</span>
5 0
3 years ago
The Answers plz and thx
garri49 [273]

Answer:

The answers to what?

Explanation:

50x89=4,450

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What do the little numbers (subscripts) next to the lower right of each letter mean in the C₂H₄O₂?
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