A sample of magnesium ribbon is ignited in a crucible to form magnesium oxide. Refer to Example Exercise 6.1 and determine the empirical formula of magnesium oxide from the following data: mass of crucible and cover + magnesium metal mass of crucible and cover mass of crucible and cover + magnesium oxide 33.741 g 33.500 g 33.899 g o to 19dm

A compound is 80.0% carbon and 20.0% hydrogen by mass. Assume a 100.-g sample of this compound.

Complete the table below for calculating the molar mass of the ionic compound zinc oxide. Formula Molar mass of ion g/mol g/mol x Cation Zn²+ Anion 0²- Number of ions mol mol = = Mass of ion in one mole of zinc oxide Molar mass zinc oxide = g g/mol

3. Elements B and N form a binary compound BNy When 12 grams of this compound was made from its elements, it consumed 7 grams of elemental nitrogen. A) Find the empirical formula of the compound: The mass of N atoms in the 12 g sample of the compound is g The number of moles of N atoms in the 12 g sample of the compound is mol The mass ofB atoms in the 12 g sample of the compound is g The number of moles of B atoms in the 12 g sample of the compound is mol The empirical formula is: B) Given the molar mass of the compound is 74.46 g/mol, find its chemical formula: Name the compound:

When 5.095 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 15.61 grams of CO₂ and 7.457 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. empirical formula molecular formula = = Previous Next

When 3.269 g of zinc is heated in pure oxygen, the sample gains 0.800 g of oxygen in forming the oxide. Calculate the empirical formula of zine oxide.