Question

Determine the molecular formula for compound hydrogen = 6.67% Carbon = 40% and the rest is oxygen

Answer 1

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We are given that the compound contains 6.67% of hydrogen, 40 % of carbon and rest oxygen.

Therefore ;

100 grams of the compound will contain 6.67 g of hydrogen,

40 g of carbon and

(100 - 40 - 6.67)g  = 53.33 g of oxygen.

Number of moles in 6.67g of hydrogen = mass of hydrogen / molar mass of hydrogen

= 6.67 / 1 = 6.67

Number of moles in 40g of carbon = 40 / 12 = 3.33

Number of moles in 53.33g of oxygen = 53.33 / 16 = 3.33

Now, we will calculate the simplest ratio of the elements by dividing the number of moles of each element by the smallest value,

that is 3.33.

Thus

we will get

Simplest ratio of elements =

C(3.33/3.33)H(6.67/3.33)O(3.33/3.33)

= CH2O

Thus the empirical formula of the substance is CH2O and therefore the empirical mass is 

= (molar mass of carbon + 2 X molar mass of hydrogen + molar mass of oxygen)

= (12 + 2 + 16)

= 30g

Now, we know that the volume of one mole of gas is 22.4 L or 22400 cm3. We are given that 0.6g of the gas weighs 224 cm3. Thus

 22400 cm3 of a gas = 1 mole

 1cm3  = (1/22400) moles

 224 cm3  = (224/22400) moles

 = 0.01 moles

This means that the mass of 0.01 moles of a gas is 0.6g. Now we also have the relation

 number of moles = mass of substance / molar mass of substance

 0.01 = 0.6 / molar mass of substance

 So molar mass of substance = 60g

Thus n = molar mass / empirical mass

= 60 / 30

= 2

So, the molecular formula of the substance will be (CH2O)2 = C2H4O2

Thanks and regards

Ajay
B.tech , IIT(BHU)Varanasi

Answer 2

Answer:

Explanation:Plzz see the attachment

Hope it helps