Determine the empirical formula of a compound containing 48.38 grams of carbon, 8.12 grams of hydrogen, and 53.5 grams of oxygen. In an experiment, the molar mass of the compound was determined to be 180.15 g/mol. What is the molecular formula of the compound?

The empirical formula would be .

Explanation:

To find the empirical formula, we will first have to convert the mass of each element to moles of each element:

(48.38 g C) (1 mol/ 12.10 g C) = 4.028 mol C

(8.12 g H) (1 mol/ 1.008 g H) = 8.056 mol H

(53.38 g O) (1 mol/ 16.00 g O) = 3.336 mol O

Next, divide the number of moles of each by the smallest number of moles to find the ratio or the moles of each element:

(3.336 mol O/ 3.336) = 1 mol O

(4.028 mol C/ 3.336) = 1.2 mol C

(8.056 mol H/ 3.336) = 2.4 mol H

Finally, let's look at the mole ratio. We have to multiply all the mole ratios by a constant to get then all to be whole numbers. In this case, 5 would be the multiplication factor needed.

(1 mol O) (5) = 5 mol O

(1.2 mol C) (5) = 6 mol C

(2.4 mol H) (5) = 12 mol H

Now, the ratios are whole numbers, and we can write the empirical formula as thus:

metals are good conductor of electricity. it has free electrons on their surface. according to electron pool theory, each atom present in a metal crystal losses all of its valence electron and as a result a pool of free is form. these pool of electrons are free to move and   conduct electricity easily   while making metal as good conductor.

the correct answer is a. the ability of electrons to flow throughout the metal.

if it's not useful, feel free to report for mistake in answer.