Calculate the molar mass of each of the following: (a) SnO (b) BaF2 (c) Al2(SO4)3 (d) MnCl2

In a combination reaction, 1.62 g of lithium is mixed with6.50 g of oxygen. (a) Which reactant is present in excess?(b) How many moles of product are formed? (c) After reaction,how many grams of each reactant and product are present?

(a) How many moles of ammonium ions are in 0.459 g of ammonium carbonate?  _______mol(b) What is the mass, in grams, of 0.0329 mol of iron(III) phosphate? ________g(c) What is the mass, in grams, of 4.90  1023 molecules of aspirin, C9H8O4?   ________g(d) What is the molar mass of a particular compound if 0.078 mol weighs 6.34 g? _________g/mol

(a) How many moles of ammonium ions are in 0.393 g of ammonium carbonate? mol (b) What is the mass, in grams, of 0.0569 mol of iron(III) phosphate? 9 (c) What is the mass, in grams, of 2.70 x 1023 molecules of aspirin, C,HgO4? 9 (d) What is the molar mass of a particular compound if 0.050 mol weighs 6.02 g? g/mol

Calculate each of the following quantities:(a) Total number of ions in 38.1 g of SrF₂(b) Mass in kilograms of 3.58 mol of CuCl₂.2H₂O(c) Mass in milligrams of 2.88x10^22 formula units of Bi(NO₃).35H₂O

(a) What is the mass, in grams, of 4.62  1023 molecules of aspirin, C9H8O4?  (b) What is the molar mass of diazepam (Valium(R)) if 0.05570 mol weighs 15.86 g?  g/mol (c) How many moles of ammonium ions are in 0.645 g of ammonium carbonate?

A sample of a substance with the empirical formula XCI2 weighs 0.5719 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 1.2191 g. The chemical reaction is XCI₂ + 2 AgNO3-2AgCl + X(NO3)2 (a) Calculate the formula mass of XCI2. Formula mass XCI2 = g mol-1 (b) Calculate the atomic mass of X. Atomic mass X = g mol-1

Compound X has a molar mass of 134.12·gmol−1 and the following composition: element mass % carbon 44.77% hydrogen 7.52% oxygen 47.72% Write the molecular formula of X .

In a reaction to produce NaF, 3.50 g of HF and 1.26 of Na2SiO3 are reacted according to the following: Na2SiO3 (s) + HF (aq) →H2SiF6 (aq) + NaF (aq) + H2O (l) (a) Balance the equation.   (b) Calculate the theoretical yield of NaF.   (c) If 0.792 g of NaF is formed, calculate the percent yield.

In a combination reaction, 1.54 g of lithium is mixed with 6.68 g of oxygen. (a) Which reactant is present in excess? (b) How many moles of product are formed? (c) After the reaction, how many grams of each reactant and product are present? Including Li2O