Complete combustion of 7.60 g of a hydrocarbon produced 23.4 g of co2 and 10.8 g of h2o. what is the empirical formula for the hydrocarbon?

Mass of hydrocarbon = 7.60 g

All the C gets converted to 23.4 g of CO2

All the H gets converted to 10.8 g of H2O

Now:

Molecular mass of CO2 = 48 g/mol

Molecular mass of H2O = 18 g/mol

# moles of CO2 = 23.4 g/48 gmol-1 = 0.4875  = moles of C

# moles of H2O = 10.8/18 = 0.6 moles = moles of H

Now:

Mass of C = 0.4875 moles * 12 g/mole = 5.85 g

Mass of H = 0.6 moles * 1 g/mole = 0.6 g

Total mass = C + H = 5.85 + 0.6 = 6.45 g. Ideally, this must be equal to the given  mass of the hydrocarbon, 7.60 g.

Nevertheless, in order to find the empirical formula, divide the # moles of C and H by the smallest value:

C = 0.4875/0.4875 = 1

H = 0.6/0.4875 = 1.23 (approximately = 1)

Empirical formula = CH

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.