Silicon tetrachloride is used in the electronics industry to make elemental silicon for computer chips. Silicon tetrachloride is prepared from silicon dioxide, graphitic carbon, and chlorine gas:

SiO2(s)+2C(s)+2Cl2(g)−−\SiCl4(l)+2CO(g)

If the reaction occurs with a 90.0% yield, what mass of silicon tetrachloride can be prepared from 51.9 g of each starting material? Enter units. Im new to chemistry and this site a friend told me i should do this since i needed help.. PLEASE HELPPP

Question

Silicon tetrachloride is used in the electronics industry to make elemental silicon for computer chips. Silicon tetrachloride is prepared from silicon dioxide, graphitic carbon, and chlorine gas:

SiO2(s)+2C(s)+2Cl2(g)−−\>SiCl4(l)+2CO(g)

If the reaction occurs with a 90.0% yield, what mass of silicon tetrachloride can be prepared from 51.9 g of each starting material? Enter units. Im new to chemistry and this site a friend told me i should do this since i needed help.. PLEASE HELPPP

anonymous · Answer

http://answers.yahoo.com/question/index?qid=20100602162644AAl9t3v same question is asked there with different value . May this help u .

aaronq · Answer

Convert 51.9 g to moles, determine which reactant you have less of (i.e. find the limiting reactant).

use those moles to build a ratio, and solve for the moles of product.

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e.g. for a general reaction:

                      $\color{red}{a}A + \color{blue}{b}B$ $\rightleftharpoons$ $ \color{green}{c}C$

where upper case are the species (A,B,C), and lower case (a,b,c) are the coefficients (in red),

                     $\dfrac{n_A}{\color{red}{a}}=\dfrac{n_B}{\color{blue}{b}}=\dfrac{n_C}{\color{green}{c}}$

from here, you can solve for moles then convert to grams.

To convert mass to moles, use the relationship:

                             $n=\dfrac{m}{M}$

        where, M=molar mass, m=mass, and n= moles.