Question

Write a balanced equation for the reaction depicted below:

If each reactant molecule represents 1.25×10^-2 mol and the reaction yield is 87%, how many grams of Si-containing product form?

Short answer

The yield of the Si-containing product form is 3.4 g SiF₄.

Step-by-step solution

Calculating the mass of SiF4

The chemical equation can be denoted as,

$3Si{H}_4+3N_2{F}_4\to 2Si{F}_4+3N_2+6H_2$

On dividing the equation by 3,

$Si{H}_4+N_2{F}_4\to Si{F}_4+N_2+2H_2$

On calculating the mass,

$$\begin{gathered} MassofSiF\left(theoretical\right)=3.75\times {10}^{-2}molSi{F}_4\times \frac{104.08Si{F}_4}{1molSi{F}_4} \\ MassofSiF\left(theoretical\right)=3.903gSi{F}_4 \end{gathered}$$

Calculating the actual yield of SiF4

The actual yield can be denoted as,

$\begin{array}{rcl}\%yieldofSi{F}_4& =& \frac{actualyieldofSi{F}_4}{theoreticalyieldofSi{F}_4}\times 100\\ ActualyieldofSi{F}_4& =& \frac{87\times 3.903gSi{F}_4}{100}\\ ActualyieldofSi{F}_4& =& 3.4gSi{F}_4\end{array}$