# Problem: A compound has the empirical formula CHCl. A 256-mL flask, at 373 K and 750. torr, contains 0.800 g of the gaseouscompound. Give the molecular formula.

🤓 Based on our data, we think this question is relevant for Professor Tang's class at USF.

###### FREE Expert Solution
• We need to find the molar mass of the empirical formula and the actual gas since this will tell us how many atoms of C, H and Cl are present in the gas and the actual molecular formula of the gas
• Molar mass of CHCl will appear as:

C - 12.01 (1) = 12.01

H - 1.01 (1) = 1.01

Cl - 35.45 (1) = 35.45

12.01 + 1.01 + 35.45 = 48.47 g/mol

• For the actual molecular formula, we will be using the ideal gas equation and use the conditions provided to find the moles
• Calculating for moles:
###### Problem Details

A compound has the empirical formula CHCl. A 256-mL flask, at 373 K and 750. torr, contains 0.800 g of the gaseous
compound. Give the molecular formula.

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Ideal Gas Law Molar Mass concept. If you need more Ideal Gas Law Molar Mass practice, you can also practice Ideal Gas Law Molar Mass practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Tang's class at USF.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl 2nd Edition practice problems.