91Ó°ÊÓ

What is the molecular formula of a compound with an empirical formula of \(\mathrm{HO}\) and a molar mass of \(34 \mathrm{~g} / \mathrm{mol}\) ?

empirical formula of \(\mathrm{HO}\) and a molar mass of \(34 \mathrm{~g} / \mathrm{mol}\) ? What is the molecular formula of each of the following compounds? (a) empirical formula of \(\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}\) and molar mass of \(132 \mathrm{~g} / \mathrm{mol}\) (b) empirical formula of \(\mathrm{C}_{3} \mathrm{H}_{4} \mathrm{NO}_{3}\) and molar mass of \(408 \mathrm{~g} / \mathrm{mol}\)

What is the molecular formula of each of the following compounds? (a) empirical formula \(\mathrm{C}_{5} \mathrm{H}_{10} \mathrm{O}\) and molar mass of \(258 \mathrm{~g} / \mathrm{mol}\) (b) empirical formula \(\mathrm{PCl}_{3}\) and molar mass of \(137.3 \mathrm{~g} / \mathrm{mol} ?\)

A compound contains \(62.0 \%\) carbon, \(10.4 \%\) hydrogen, and \(27.5 \%\) oxygen by mass, and has a molar mass of \(174 \mathrm{~g} / \mathrm{mol}\). What is the molecular formula of the compound?

Mandelic acid is an organic acid composed of carbon \((63.15 \%)\), hydrogen \((5.30 \%)\), and oxygen \((31.55 \%)\). Its molar mass is \(152.14 \mathrm{~g} / \mathrm{mol}\). Determine the empirical and molecular formulas of the acid.

Acetic acid gives vinegar its sour taste. Analysis of acetic acid shows it is \(40.0 \%\) carbon, \(6.71 \%\) hydrogen, and \(53.3 \%\) oxygen. Its molar mass is \(60 \mathrm{~g} / \mathrm{mol}\). What is its molecular formula?

Fructose, an important sugar, is made up of \(40.0 \%\) carbon, \(6.71 \%\) hydrogen, and \(53.3 \%\) oxygen. Its molar mass is \(180 \mathrm{~g} / \mathrm{mol}\). What is its molecular formula?

(a) Write the equation for the combustion of propylene, \(\mathrm{C}_{3} \mathrm{H}_{6}\) (b) Calculate the mass of \(\mathrm{CO}_{2}\) produced when \(2.45 \mathrm{~g}\) \(\mathrm{C}_{3} \mathrm{H}_{6}\) burns in excess oxygen.

(a) Write the equation for the combustion of \(\mathrm{C}_{4} \mathrm{H}_{8} \mathrm{O}\). (b) Calculate the mass of \(\mathrm{O}_{2}\) consumed in the combustion of a \(5.33-\mathrm{g}\) sample of \(\mathrm{C}_{4} \mathrm{H}_{8} \mathrm{O}\)

What mass of \(\mathrm{NH}_{3}\) forms from the reaction of \(5.33 \mathrm{~g} \mathrm{~N}_{2}\) with excess \(\mathrm{H}_{2} ?\)