A compound contains 4.07 % hydrogen, 24....

A compound contains 4.07 % hydrogen, 24.27% carbon and 71.65% chlorine. Its molecular mass is 98.96. What are its empirical and molecular formulae ?

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To find the empirical and molecular formulas of the compound, we will follow these steps: ### Step 1: Assume a Sample Mass Assume a sample mass of 100 grams of the compound. This makes calculations straightforward since the percentages can be directly interpreted as grams. ### Step 2: Calculate the Mass of Each Element From the given percentages: - Mass of Hydrogen (H) = 4.07% of 100 g = 4.07 g ...

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A compound contains 4.2% hydrogen, 24.2% carbon and 71.6% chlorine by mass. Its molar mass is 98.96 gm//mol . Empirical formula of compound is :

`CH_(2)CI`

`C_(2)H_(4)CI_(2)`

`C_(2)H_(2)CI_(2)`

`C_(4)H_(4)CI_(4)`

A compound contains 4.07% H, 24.27% C , and 71.65% Cl . If its molar mass is 98.96 , the molecular formula will be

`C_(2) H_(4) Cl_(2)`

`CH_(2) Cl`

`C_(3) H_(6) H_(3)`

`C_(4) H_(8) Cl_(4)`

A carbon compound contains 12.8% of carbon, 2.1% of hydrogen and 85.1% bromine . The molecule mass of compound is 187.9. calculate the molecular formula of the compound (Atomic mass H=1.008,C=12,Br=79.9)

`CH_(3)Br`

`CH_(2)Br_(2)`

`C_(2)H_(4)Br_(2)`

`C_(2)H_(3)Br_(3)`