When 3.869 grams of a hydrocarbon, C_xH_y, were burned in a combustion analysis apparatus, 11.86 grams of CO₂ and 5.664 grams of H₂O were produced. In a separate experiment, the molar mass of the compound was found to be 86.18 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon.

Enter the elements in the order presented in the question.

When 5.914 grams of a hydrocarbon, C_xH_y, were burned in a combustion analysis apparatus, 19.99 grams of CO₂ and 4.092 grams of H₂O were produced. In a separate experiment, the molar mass of the compound was found to be 26.04 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon.

A 23.71 gram sample of cobalt is heated in the presence of excess oxygen. A metal oxide is formed with a mass of 33.37 g. Determine the empirical formula of the metal oxide.

Enter the elements in the order Co, O

A sample of a substance with the empirical formula XCl₂ weighs 0.4523 g. When it is dissolved in water and all its chlorine is converted to insoluble AgCl by addition of an excess of silver nitrate, the mass of the resulting AgCl is found to be 0.9985 g. The chemical reaction is

XCl₂ + 2 AgNO₃2AgCl + X(NO₃)₂

(a) Calculate the formula mass of XCl₂.

Formula mass XCl₂ = ? g mol^-1

(b) Calculate the atomic mass of X.

Atomic mass X = ? g mol^-1