Question

One of relatively few reactions that takes place directly between two solids at room temperature is In this equation, the in Ba(OH)2 indicates the presence of eight water molecules. This compound is called barium hydroxide octahydrate.

a. Balance the equation.
b. What mass of ammonium thiocyanate (NH4SCN) must be used if it is to react completely with 6.5 g barium hydroxide octahydrate?

Answer 1

3.14 grams of ammonium thiocyanate must be used to react completely with 6.5 g barium hydroxide octahydrate.

Step-by-step explanation:

`Ba(OH)_2.8H_2O(s)+NH_4SCN(s)\rightarrow Ba(SCN)_2(s)+8H_2O(l)+NH_3(g)`

The balance chemical equation is :

`Ba(OH)_2.8H_2O(s)+2NH_4SCN(s)\rightarrow Ba(SCN)_2(s)+10H_2O(l)+2NH_3(g)`

Mass of barium hydroxide octahydrate = 6.5 g

Moles of barium hydroxide octahydrate =
`(6.5 g)/(315 g/mol)=0.020635 mol`

According to reaction, 2 moles of ammonium thiocyanate reacts with1 mole of barium hydroxide octahydrate. The 0.020635 moles of barium hydroxide octahydrate will react with:

`(2)/(1)* 0.020635 mol=0.04127 mol`

Mass of 0.04127 moles of ammonium thiocyanate;

`0.04127 mol* 76 g/mol=3.136 g\approx 3.14 g`

3.14 grams of ammonium thiocyanate must be used to react completely with 6.5 g barium hydroxide octahydrate