Chemistry problems that need an answer please?

Question

One of relatively few reactions that takes place directly between two solids at room temp. is: Ba(OH)2*8H2O+NH4SCN(s) yields Ba(SCN)2(s) + H2O(l) + NH3 (g)

In the equation the *H2O in Ba(OH02*8H2O indicates the prescence of eight water molecules. This compound is called barium hydroxide octahydrate.

a) Balance the equation.

b) What mass of ammonium thiocyanate must be used if it is to react completely with 6.5 g barium hydroside octahydrate?

c) What masses of the three products would be produced in the reaction of part b?

Answer 1

a)  Ba(OH)2 * 8H2O + _2_NHSCN(s) -> Ba(SCN)2(s) + _10_H2O(l) + _2_NH3 (g)

b) Find Molar mass of barium hydroxide octahydrate. Find how many moles are in 6.5g.  Refer back to the balanced equation to see how many moles of ammonium thiocyanate react completely with however many moles you just found (multiply by the ratio, its 2).  Convert moles to grams (using molar mass of ammonium thiocyanate) for mass. I believe the answer is 3.14 g.

c) Relate how many moles you used for the reactants to the moles of the products and convert to grams using the molar mass of each product.  

Ba(SCN)2- .0206 mol, H20- .206 mol, NH3- .0412 mol (convert to grams)