Q145CP - Chemistry: Molecular Nature Of Matter And Change

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?

Step-by-Step Solution

Answer

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

Step 1: Calculating the mass of SiF 4

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,

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

Step 2: Calculating the actual yield of SiF 4

The actual yield can be denoted as,

$\begin{array}{rcl}\%yield of Si{F}_4& =& \frac{actualyield of Si{F}_4}{theoreticalyield of Si{F}_4}\times 100\\ Actual yield of Si{F}_4& =& \frac{87\times 3.903gSi{F}_4}{100}\\ Actual yield of Si{F}_4& =& 3.4gSi{F}_4\end{array}$