Complete combustion of 3.90 g of a hydrocarbon produced 12.5 g of co2 and 4.28 g of h2o. what is the empirical formula for the hydrocarbon?

Empirical formula of the hydrocarbon is .

Explanation:

Mass of carbon dioxide produced = 12.5 g

Moles of carbon dioxide =

Moles of carbon atom in 0.2841 moles of carbon dioxide:

1 × 0.2841 mol = 0.2841 mol

Mass of water produced = 4.28 g

Moles of water =

Moles of hydrogen in water = 2 × 0.2378 mol = 0.4756 mol

For empirical formula divide the moles of element which are is less amount with all the moles of every element.

Carbon =

Hydrogen =

Empirical formula of the hydrocarbon is .

in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm

answer: enthalpy

explanation:

for a exothermic reaction, the energy is released i.e. the energy of the products is lower than the energy of the reactants.

= enthaply

= energy of products

= energy of reactants

as , thus comes out to be negative. negative value of enthalpy shows that the reaction is exothermic.