An unknown compound comprised of osmium and chlorine is 40.11% osmium by mass. a. If you assume 100.0 g of the compound, what is the mass in grams of osmium that are present in the compound? b. How many moles of osmium are present in 100.0 g of the compound? c. If you assume 100.0 g of the compound, what is the mass in grams of chlorine that are present in the compound?

What amount (moles) is represented by each of these samples? a. 102.9 g Fe2O3 mol b. 34.6 mg NO2 mol c. 6.1 x 1016 molecules of BF3 mol

a. A compound is 54.53% C, 9.15% H, and 36.32% O by mass. What is its empirical formula? b. The molecular mass of a compound is 132 amu. What is its molecular formula?

1A. You have 33.5g MnO3. How many molecules do you have?1B. You have 4.6x1024 molecules O2. How many grams do you have?1C. You have 6.54x1022 molecules Fe2O3. How many grams do you have?1D. You have 43.2g of Cobalt. How many atoms do you have?

b. If 1.530 g of copper (II) chloride reacts completely with 5.210 g of sodium carbonate, how much copper (II) carbonate can be formed when reaction completed?

Mass of H20 is 2.9445 g Mass of CO2 is 7.1918 g Moles of H20 is 0.1634 Moles of CO2 is 0.1634 Determine the Moles and Mass of H, C, O atoms

D. Calculate the mass (g) of the following samples. 25) 238 moles of lead 26) 1.54 x 10⁹ moles of Zn 27) 7.70 x 10-⁹ moles of Mg(NO3)2 28) 8.42 x 1027 atoms of tin 29) 6.39 x 10¹8 atoms of sulfur 30) 5.99 x 1030 molecules of SiO₂

Elements B and N form a binary compound BxNy. 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 of B 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:

2.50 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 138. g/mol, is burned completely in excess oxygen, and the mass of the products carefully measured: product 4 carbon dioxide 0 water Use this information to find the molecular formula of X. mass 5.58 g 0.98 g S A

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: