- #1
Kiah Palmer
- 8
- 3
- Homework Statement
- In the first step of silicon purification, a reaction is brought about between the impure silicon and chlorine. Pure silicon is then used, in the computer industry, for the manufacture of microchips.
Si + Cl2 -> SiCl4 (unbalanced equation)
Given that the silicon is 92% pure, calculate the theoretical yield percentage if 1.0 t of impure silicon produces 2.33 t of silicon (IV) chloride.
- Relevant Equations
- (Balanced Equation) Si + 2Cl2 -> SiCl4
Conversion: 1.0 t = 1.0x10^6 g impure Si
Conversion: 2.33 t = 2.33x10^6 g SiCl4
Atomic Mass Si = 28.085 g/mol
Atomic Mass Cl2 = (2 x 35.453) = 70.906 g/mol
Mass SiCl4 = 28.085 + (4x35.453) = 169.897 g/molI got all this part down, however, I'm not quite sure where I am supposed to go from there...
Conversion: 2.33 t = 2.33x10^6 g SiCl4
Atomic Mass Si = 28.085 g/mol
Atomic Mass Cl2 = (2 x 35.453) = 70.906 g/mol
Mass SiCl4 = 28.085 + (4x35.453) = 169.897 g/molI got all this part down, however, I'm not quite sure where I am supposed to go from there...