Solved

The Integrated Circuits in Your Cell Phone and Computer Are $\Delta$

Question 83

Multiple Choice

The integrated circuits in your cell phone and computer are made from the semiconductor silicon. The silicon is obtained from a really inexpensive starting material, sand, which is primarily SiO₂. One step in the purification of silicon is to separate it from solid impurities by forming the gas silicon tetrachloride. Given the following reactions, what is the overall enthalpy change in converting 1.00 mol of silicon dioxide into pure silicon? Reaction $\Delta$ H^$\circ$ (kJ)
SiO₂(s) $The integrated circuits in your cell phone and computer are made from the semiconductor silicon. The silicon is obtained from a really inexpensive starting material, sand, which is primarily SiO2. One step in the purification of silicon is to separate it from solid impurities by forming the gas silicon tetrachloride. Given the following reactions, what is the overall enthalpy change in converting 1.00 mol of silicon dioxide into pure silicon? Reaction \Delta H \circ (kJ) SiO2(s) 2C(s) Si(impure s) 2CO(g) +690 Si(impure s) 2Cl2(g) SiCl4(g) -657 SiCl4(g) 2Mg(s) 2MgCl2(s) Si(s) -625 A) (+1,972 kJ) B) (-1,972 kJ) C) (-592 kJ) D) (+592 kJ) E) (-625 kJ)$ 2C(s) $The integrated circuits in your cell phone and computer are made from the semiconductor silicon. The silicon is obtained from a really inexpensive starting material, sand, which is primarily SiO2. One step in the purification of silicon is to separate it from solid impurities by forming the gas silicon tetrachloride. Given the following reactions, what is the overall enthalpy change in converting 1.00 mol of silicon dioxide into pure silicon? Reaction \Delta H \circ (kJ) SiO2(s) 2C(s) Si(impure s) 2CO(g) +690 Si(impure s) 2Cl2(g) SiCl4(g) -657 SiCl4(g) 2Mg(s) 2MgCl2(s) Si(s) -625 A) (+1,972 kJ) B) (-1,972 kJ) C) (-592 kJ) D) (+592 kJ) E) (-625 kJ)$ Si(impure s) $The integrated circuits in your cell phone and computer are made from the semiconductor silicon. The silicon is obtained from a really inexpensive starting material, sand, which is primarily SiO2. One step in the purification of silicon is to separate it from solid impurities by forming the gas silicon tetrachloride. Given the following reactions, what is the overall enthalpy change in converting 1.00 mol of silicon dioxide into pure silicon? Reaction \Delta H \circ (kJ) SiO2(s) 2C(s) Si(impure s) 2CO(g) +690 Si(impure s) 2Cl2(g) SiCl4(g) -657 SiCl4(g) 2Mg(s) 2MgCl2(s) Si(s) -625 A) (+1,972 kJ) B) (-1,972 kJ) C) (-592 kJ) D) (+592 kJ) E) (-625 kJ)$ 2CO(g) +690
Si(impure s) $The integrated circuits in your cell phone and computer are made from the semiconductor silicon. The silicon is obtained from a really inexpensive starting material, sand, which is primarily SiO2. One step in the purification of silicon is to separate it from solid impurities by forming the gas silicon tetrachloride. Given the following reactions, what is the overall enthalpy change in converting 1.00 mol of silicon dioxide into pure silicon? Reaction \Delta H \circ (kJ) SiO2(s) 2C(s) Si(impure s) 2CO(g) +690 Si(impure s) 2Cl2(g) SiCl4(g) -657 SiCl4(g) 2Mg(s) 2MgCl2(s) Si(s) -625 A) (+1,972 kJ) B) (-1,972 kJ) C) (-592 kJ) D) (+592 kJ) E) (-625 kJ)$ 2Cl₂(g) $The integrated circuits in your cell phone and computer are made from the semiconductor silicon. The silicon is obtained from a really inexpensive starting material, sand, which is primarily SiO2. One step in the purification of silicon is to separate it from solid impurities by forming the gas silicon tetrachloride. Given the following reactions, what is the overall enthalpy change in converting 1.00 mol of silicon dioxide into pure silicon? Reaction \Delta H \circ (kJ) SiO2(s) 2C(s) Si(impure s) 2CO(g) +690 Si(impure s) 2Cl2(g) SiCl4(g) -657 SiCl4(g) 2Mg(s) 2MgCl2(s) Si(s) -625 A) (+1,972 kJ) B) (-1,972 kJ) C) (-592 kJ) D) (+592 kJ) E) (-625 kJ)$ SiCl₄(g) -657
SiCl₄(g) $The integrated circuits in your cell phone and computer are made from the semiconductor silicon. The silicon is obtained from a really inexpensive starting material, sand, which is primarily SiO2. One step in the purification of silicon is to separate it from solid impurities by forming the gas silicon tetrachloride. Given the following reactions, what is the overall enthalpy change in converting 1.00 mol of silicon dioxide into pure silicon? Reaction \Delta H \circ (kJ) SiO2(s) 2C(s) Si(impure s) 2CO(g) +690 Si(impure s) 2Cl2(g) SiCl4(g) -657 SiCl4(g) 2Mg(s) 2MgCl2(s) Si(s) -625 A) (+1,972 kJ) B) (-1,972 kJ) C) (-592 kJ) D) (+592 kJ) E) (-625 kJ)$ 2Mg(s) $The integrated circuits in your cell phone and computer are made from the semiconductor silicon. The silicon is obtained from a really inexpensive starting material, sand, which is primarily SiO2. One step in the purification of silicon is to separate it from solid impurities by forming the gas silicon tetrachloride. Given the following reactions, what is the overall enthalpy change in converting 1.00 mol of silicon dioxide into pure silicon? Reaction \Delta H \circ (kJ) SiO2(s) 2C(s) Si(impure s) 2CO(g) +690 Si(impure s) 2Cl2(g) SiCl4(g) -657 SiCl4(g) 2Mg(s) 2MgCl2(s) Si(s) -625 A) (+1,972 kJ) B) (-1,972 kJ) C) (-592 kJ) D) (+592 kJ) E) (-625 kJ)$ 2MgCl₂(s) $The integrated circuits in your cell phone and computer are made from the semiconductor silicon. The silicon is obtained from a really inexpensive starting material, sand, which is primarily SiO2. One step in the purification of silicon is to separate it from solid impurities by forming the gas silicon tetrachloride. Given the following reactions, what is the overall enthalpy change in converting 1.00 mol of silicon dioxide into pure silicon? Reaction \Delta H \circ (kJ) SiO2(s) 2C(s) Si(impure s) 2CO(g) +690 Si(impure s) 2Cl2(g) SiCl4(g) -657 SiCl4(g) 2Mg(s) 2MgCl2(s) Si(s) -625 A) (+1,972 kJ) B) (-1,972 kJ) C) (-592 kJ) D) (+592 kJ) E) (-625 kJ)$ Si(s) -625