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Verdich [7]
3 years ago
7

Calculate the empirical formula of a compound that is 42.9% Carbon and 57.1% Oxygen.

Chemistry
1 answer:
Marrrta [24]3 years ago
4 0

Answer:

CO.

Explanation:

Assuming the given percentages are by mass, we can solve this problem via imagining we have <em>100 g of the compound</em>, if that were the case we would have:

  • 42.9 g of C
  • 57.1 g of O

Now we <u>convert those masses into moles</u>, using the<em> elements' respective molar masses</em>:

  • 42.9 g of C ÷ 12 g/mol =  3.57 mol C
  • 57.1 g of O ÷ 16 g/mol =  3.58 mol O

As the number of C moles and O moles is roughly the same, the empirical formula for the compound is <em>CO</em>.

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Answer:

Explanation:

The atomic radius of elements are used to estimate the sizes of elements. The atomic radius is taken as half of the inter-nuclear distance between two covalently bonded atoms of non-metallic elements or half of the distance between two nuclei in the solid state of metals.

To solve this problem we will obtain the atomic radius values of the given elements from a standard atomic radius table;

          Si          111 pm

           P          98 pm

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pm = picometer

We see that chlorine has the least atomic radius

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4 years ago
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3 years ago
In order to keep the bench from conducting heat, Shane could build it out of _______.
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✧・゚: *✧・゚:*    *:・゚✧*:・゚✧

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~ ʜᴏᴘᴇ ᴛʜɪꜱ ʜᴇʟᴘꜱ! :) ♡

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How many milliliters of 0.150 M NaOH are required to neutralize 85.0 mL of 0.300 M H2SO4 ? The balanced neutralization reaction
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Answer : The volume of NaOH required to neutralize is, 340 mL

Explanation :

To calculate the volume of base (NaOH), we use the equation given by neutralization reaction:

n_1M_1V_1=n_2M_2V_2

where,

n_1,M_1\text{ and }V_1 are the n-factor, molarity and volume of acid which is H_2SO_4

n_2,M_2\text{ and }V_2 are the n-factor, molarity and volume of base which is NaOH.

We are given:

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2\times 0.300M\times 85.0mL=1\times 0.150M\times V_2\\\\V_2=340mL

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