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

1 answer:

6 0

The reaction equation is:
Ba(OH)₂*8H₂O + 2NH₄SCN(s) → Ba(SCN)₂(s) + 10H₂O(l) + 2NH₃ (g)

The molecular mass of barium hydroxide octahydrate is 315 grams /mol.
We determine the number of moles of barium hydroxide octahydrate:
moles = mass / Mr
moles = 6.5 / 315
moles = 0.02 mol

Using the equation, we can determine that the moles of ammonium thiocyanate required are:
2 * 0.02 = 0.04 mol

The molecular weight of ammonium thiocyanate is 76.1 grams / mol

Weight = moles * Mr
Weight = 0.04 * 76.1
Weight = 3.04 grams

3.04 grams of ammonium thicyanate are required.

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New questionWhat mass of calcium chloride (CaCl₂) would beproduced from the reaction of 125.9 g of hydrochloriacid (HCI) with ex

marshall27 [118]

Answer:

191.6 g of CaCl₂.

Explanation:

What is given?

Mass of HCl = 125.9 g.

Molar mass of CaCl₂ = 110.8 g/mol.

Molar mass of HCl = 36.4 g/mol.

Step-by-step solution:

First, we have to state the chemical equation. Ca(OH)₂ react with HCl to produce CaCl₂:

$Ca(OH)_2+2HCl\rightarrow CaCl_2+2H_2O.$

Now, let's convert 125.9 g of HCl to moles using the given molar mass (remember that the molar mass of a compound can be found using the periodic table). The conversion will look like this:

$125.9\text{ g HCl}\cdot\frac{1\text{ mol HCl}}{36.4\text{ g HCl}}=3.459\text{ moles HCl.}$

Let's find how many moles of CaCl₂ are being produced by 3.459 moles of HCl. You can see in the chemical equation that 2 moles of HCl reacted with excess Ca(OH)₂ produces 1 mol of CaCl₂, so we state a rule of three and the calculation is: