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Sergio [31]
3 years ago
9

#12, how do I solve this

Chemistry
1 answer:
Likurg_2 [28]3 years ago
5 0
Find the molar mass of the compound, then get the unit cancel out until u reach "g"

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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
Use of chemical substance in our daily life their advantages and disadvantages​
vekshin1

Answer:

Explanation:

By observing chemical reactions, we are able to understand and explain how the natural world works. Chemical reactions turn food into fuel for your body, make fireworks explode, cause food to change when it is cooked, make soap remove grime, and much more.

3 0
3 years ago
In the equilibrium and concentration gizmo, you learned that you can predict the direction of a reaction by comparing the reacti
max2010maxim [7]

And the significant amount of volume can be differed by its solitude

4 0
3 years ago
Complete combustion of 3.20g of a hydrocarbon produced 9.69g of CO2 and 4.96g of H2O. What is the empirical formula for the hydr
vlabodo [156]

Let empirical formula for hydrocarbon is CxHy

it will undergo combustion as

CxHy + (x + y/4) O2  ---> xCO2 + (y/2 )H2O

Given that mass of CO2 produced = 9.69 g

So moles of CO2 produced = 9.69 / 44 = 0.22 moles

So moles of carbon present = 0.22 moles

mass of H2O produced = 4.96 g

Moles of H2O produced = mass / molar mass = 4.96 / 18 = 0.28 moles

So moles of H present = 2 X 0.28 = 0.56 moles

Let us divided the moles of each with lowest value of moles

Moles of Carbon = 0.22 / 0.22 = 1 moles

moles of H = 0.56 / 0.22 = 2.55

Multiplying with two to get whole number

the ratio of carbon and hydrogen will be : C:H = 2:5

empirical formula : C2H5


4 0
3 years ago
Read 2 more answers
How many grams of CO are produced when 41.0 g of C reacts?
CaHeK987 [17]

Answer:

95.7 g CO to the nearest tenth.

Explanation:

2C + O2 ---> 2CO

Using relative atomic masses:

24 g C produces  2*12 + 2*16 g CO.

So 41 g produces  ( (2*12 + 2*16) * 41  ) / 24

= 95.7 g CO,

7 0
3 years ago
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