Question

1. Silicon nitride is made by a combining silicon and nitrogen gas (N2) at a high temperature. How much (in gram) silicon is needed to react with an excess of nitrogen gas to prepare 125 g of silicon nitride if the percent yield of the reaction is 95.0%?

Answer 1

Answer:

Silicon nitride (si3n4) is made by acombining si and nitrogen gas (n2) at a high temperature. how much (in g) si is needed to react with an excess ofnitrogen gas to prepare 125 g of silicon nitride if the percent yield of the reaction is 95.0%

Explanation:

% yield =( actual yield /theoretical yield ) *100

theoretical yield = (actual yield / % yield) *100 = (125 /85) *100 = 147.06 g Si3N4

Mole ratio of Si : Si3N4 = 3 :1

Grams of Si required to produce 147.06 g Si3N4 =

( 3 mole Si /1 mol Si3N4) ( 28.05 g Si /1 mole Si) * (1mole Si3 N4 /140.3 g Si3N4) *147.06 g Si3N4

= 88.20 g g Si (answer)