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Llana [10]
3 years ago
11

A compound containing phosphorus and oxygen has a molar mass of 219.9 g/mol and an empirical formula of p2o3. Determine its mole

cular formula.
Chemistry
1 answer:
Softa [21]3 years ago
7 0

Answer:

P₄O₆

Explanation:

The molecular formula is a whole number multiple of the empirical formula. that is, if the mole wt is 219.9 gms/mole and the empirical formula weight is 110 gms/mole*, then the whole number multiple is 219.9/110 = 2 => Molecular formula => (P₂O₄)₂ => P₄O₆.

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If 16.4 grams of calcium nitrate is heated as shown in the reaction:
vfiekz [6]

Answer:

7.2

Explanation:

you first have to find the number of moles of nitrogen dioxide by using the number of moles for calcium nitrate and the mole to mole ratios

number of moles of calcium nitrate=mass/mm

=16.4/102

=0.16g/mol

then you use the mole to mole ratios

2 : 4

0.16: x

2x/2=0.64/2

x=0.32g/moles of nitrogen dioxide

then you use the formula for the volume

v=22.4n

=22.4×0.32

=7.2

I hope this helps

4 0
2 years ago
How many of the electrons in a molecule of ethane are not involved in bondind​
vovikov84 [41]

Ethane consists of 6C−H bonds and 1C−C bond. Total number of bonds is 7. Each bond is made up of two electrons

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7 0
2 years ago
when 10.00 g of phosphorus reacts with oxygen, it produces 17.77 g of a phosphorus oxide. This phosphorus oxide was found to hav
Alex_Xolod [135]

Answer:

Molecular formula = P₄O₆

Explanation:

P(s)         +        O₂(g)------------------------------------⇒ PₓOₙ (g)

10g                     (17.77-10)g                                    17.77g

10g                        7.77g                                          17.77g  (gramme ratio)

The molecular mass of Phosphorus  (P) = 31g/mole

The molecular mass of Oxygen atom (O) = 16g/mole

Mole ratio is given by:

P              :             O

10/31                    7.77/16

0.3226       :         0.4856                Mole ratio---------------------------- (1)

Divide (1)  through by 0.3226

 1                 :        1.5-------------------------------------------- (2)

From  (2), the empirical formula for Phosphorus oxide :

Empirical formula = P₁O₁.₅

                               =  PO₁.₅

The molecular formula can be calculated from below:

Since the molecular formula is a multiple of the empirical formula we have

Molecular formula = (PO₁.₅)ₙ----------------------------------- (3)

Since we are given the molecular mass of the oxide formed, we have:

(PO₁.₅)ₙ = 220-----------------------------(4)

[31 + (16 x 1.5)] x n = 220

[31 + 24]n = 220

55n =220

n = 4

Substituting into (3), we have :

Molecular formula = (PO₁.₅)₄

                               = P₄O₆

8 0
3 years ago
For the reaction below, if the rate of appearance of Br2 is 0.180 M/s, what is the rate of disappearance of
brilliants [131]

Answer:

–0.360 M/s

Explanation:

7 0
3 years ago
An organism that regulates its body temperature using external heat sources is an example of
katovenus [111]
A cold-blooded animal. Cold-blooded animals can't generate heat themselves so they have to use external sources to keep them warm.
6 0
3 years ago
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