Home
Class 10
CHEMISTRY
A compound was found to have 78.2% boron...

A compound was found to have 78.2% boron and 21.8% of hydrogen. Its molar mass was determined to be 27.6 g `mol^(-1)`. What is the empirical and molecular formula of the compound.

Text Solution

AI Generated Solution

To determine the empirical and molecular formula of the compound with 78.2% boron and 21.8% hydrogen, follow these steps: ### Step 1: Convert Percentage to Mass Assume we have 100 grams of the compound. This means: - Mass of Boron (B) = 78.2 g - Mass of Hydrogen (H) = 21.8 g ### Step 2: Calculate Moles of Each Element ...
Promotional Banner

Topper's Solved these Questions

  • MOLE CONCEPT, STOICHIOMETRY AND BEHAVIOUR OF GASES

    MTG IIT JEE FOUNDATION|Exercise SOLVED EXAMPLES |13 Videos

  • MOLE CONCEPT, STOICHIOMETRY AND BEHAVIOUR OF GASES

    MTG IIT JEE FOUNDATION|Exercise EXERCISE (MCQ)|50 Videos

  • METALS AND NON METALS

    MTG IIT JEE FOUNDATION|Exercise Olympiad/HOTS Corner|20 Videos

  • PERIODIC CLASSIFICATION OF ELEMENTS

    MTG IIT JEE FOUNDATION|Exercise Olympiad/HOTS Corner|15 Videos

Similar Questions

Explore conceptually related problems

An organic compound having C,H and O has 13.13 % H, 52.14% C, and 34.73% O.. its molar mass is 46.068 g mol ^(-1) . What are its empirical and molecular formulae ?

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

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 ?

A gaseous compound is composed of 85.7% by mass carbon and 14.3% by mass hydrogen. Its density is 2.28 g/litre at 300 K and 1.0 atm pressure. Determine the molecular formula of the compound.

The molecular mass of a compound having empirical formula C_2H_5O is 90. The molecualr formula of the compound is:

A compound contains C=40%,O=53.5% , and H=6.5% the empirical formula formula of the compound is: