When 5.467 grams of compound z are burned in excess oxygen, 15.02 grams of co2 and 2.458 grams of h2o are produced. determine its empirical formula?

Given the mass of CO2 =15.02 g

Moles of =

Mass of H2O = 2.458 g

Moles of =

Moles of C =

Moles of H =

Mass of C in the sample =

Mass of H = =0.275 gH

Mass of O in the sample = 5.467 g - (4.095 g +0.275 g) = 1.097 g O

Moles of O =

Simplest mole ratios of the elements in the compound:

Therefore the empirical formula of the compound is

a gas, having a molecular weight of 13 kg/kmol and a kinematic viscosity of 0.25 cm2/s, flows through a pipe 0.25 m internal diameter and 5 km long at the rate of 0.4 m3/s and is delivered at atmospheric pressure.

i believe the answer is true.