Calculate the number of moles in the following quantities: a.)3.12 g NaHCO3 b.)570 mg ZnCl2 c.)8.9 x 1024 molecules CO2 d.)270 mL C2H5OH (d = 0.789 g/mL)

Please don't handwrite  solution.

5) _NH3 + 02> _NO + H20 0.3359 mol of ammonia will make how many grams of nitrogen monoxide?

mass Zn - x hort Find mass of Zn (65.4g2n) mole Zn X=9.495 * 10-3 OffS

CH3 ڈے Br 1. Mg 2. O H 3. H+/H₂O 1. Na, CH₂OH NH3 2. excess LIAIH4

A. What is the mass of CO2 produced when 15.2 g of O2 reacts with 13.0 g of C7H12? C7H12 (l) + 10 O2 (g)   ---- 7CO2 (g) + 6 H2O(g) ______  g

What is the elements, atomic mass, number of atoms, subtotal and composition? 1. Compound: C8H10N4O2   2. Compound: CuSO4 * 5 H2O

Unknow A sample ( given density= 0.795 grams/mL) Volume:24.6mL #of moles in sample:0.31825 moles Find the mass, molar mass, and number of molecules in sample.

1. Ammonium chlorate is an unstable explosive that also happens to be highly soluble in water. It is obtained by reacting barium chlorate or calcium chlorate to obtain ammonium chlorate and precipitate. a. Write out the formula for ammonium chlorate and determine the molecular weight. b. If a sample of the compound weighs 49.3 g, how many moles of oxygen atoms are there? c. How many molecules of ammonium chlorate are present in this 49.3 g sample?

An organic compound has a gram molecular weight of 372 g/mol, and its composition is 38.6% carbon, 9.76% hydrogen, and 51.56% oxygen. Determine (a) the empirical formula (b) the molecular formula.   C H O Mass of element (in g) (assuming 100 g of compound) 1._38.6_ 2._9.76__ 3._51.56_ Moles of element 4.______ 5.______ 6.______ Moles of element/Smallest moles 7.______ 8.______ 9.______ Multiplier 10._____ 10._____ 10.______ Empirical formula 11._____     Molecular weight of empirical formula 12._____     Molecular weight of compound / Molecular weight of empirical formula 13._____     True formula = C12H36O12