Question

Consider the following balanced equation: SiO2(s)+3C(s)→SiC(s)+2CO(g) Complete the following table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, as well as the moles of each product formed. If the number of moles of a product is provided, fill in the required amount of each reactant to make that amount of product, as well as the amount of the other product that is made.

Mol SiO2 Mol C Mol SiC Mol CO

Row 1: 3 _____ _____ _____

Row 2: _____ 6 _____ _____

Row 3: _____ _____ _____ 16

Row 4: 2.8 _____ _____ _____

Row 5: _____ 2.45 _____ _____

A. complete the first row. Express your answers using one significant figure separated by commas. Mol C, Mol SiC, Mol CO =

B. Complete the second row. Express your answers using one significant figure separated by commas. Mol SiO2, Mol SiC, Mol CO =

C. Complete the third row. Express your answers using two significant figures separated by commas. Mol SiO2, Mol C, Mol SiC =

D. Complete the fourth row. Express your answers using two significant figures separated by commas. Mol SiO2, Mol C, Mol SiC =

E. Complite the fifth row. Express your answers using three significant figures separated by commas. Mol SiO2, Mol SiC, Mol CO =

Answer 1

Answer:

              mol(SiO₂)              mol(C)               mol(SiC)                    mol(CO)

Row 1:      0.8 x 10               0.9 x 10              0.3 x 10                     0.6 x 10

Row 2:     0.2 x 10               0.6 x 10              0.2 x 10                     0.4 x 10

Row 3:         8.0                   2.4 x 10                   8.0                        1.6 x 10

Row 4:         2.8                      8.4                        2.8                            5.6

Row 5:        0.816                  2.45                      0.816                         1.63

Explanation:

• From the balanced equation:

SiO₂(s) + 3C(s) → SiC(s) + 2CO(g),

It is clear that 1.0 mole of SiO₂ reacts with 3.0 moles of C to produce 1.0 mole of SiC and 2.0 moles of CO.

• We can complete the table of no. of moles of each component:

A. complete the first row. Express your answers using one significant figure separated by commas. Mol C, Mol SiC, Mol CO =

3.0 moles of SiO₂:

We use the triple amount of SiO₂, so we multiply the others by 3.0.

So, it will be 3.0 moles of SiO₂ with 9.0 moles of C that produce 3.0 moles of SiC and 6.0 moles of CO.

B. Complete the second row. Express your answers using one significant figure separated by commas. Mol SiO2, Mol SiC, Mol CO =

6.0 mole of C:

We use the double amount of C, so we multiply the others by 2.0.

So, it will be 2.0 moles of SiO₂ with 6.0 moles of C that produce 2.0 moles of SiC and 4.0 moles of CO.

C. Complete the third row. Express your answers using two significant figures separated by commas. Mol SiO2, Mol C, Mol SiC =

16.0 moles of CO:

We use the amount of CO higher by 8 times than that in the balanced equation, so we multiply the others by 8.0.

So, it will be 8.0 moles of SiO₂ with 24.0 moles of C that produce 8.0 moles of SiC and 16.0 moles of CO.

D. Complete the fourth row. Express your answers using two significant figures separated by commas. Mol SiO2, Mol C, Mol SiC =

2.8 moles of SiO₂:

We use the amount of SiO₂ higher by 2.8 times than that in the balanced equation, so we multiply the others by 2.8.

So, it will be 2.8 moles of SiO₂ with 8.4 moles of C that produce 2.8 moles of SiC and 5.6 moles of CO.

E. Complite the fifth row. Express your answers using three significant figures separated by commas. Mol SiO2, Mol SiC, Mol CO =

2.45 moles of C:

We use the amount of C lower by 0.8167 times than that in the balanced equation, so we multiply the others by 0.8167.

So, it will be 0.8167 moles of SiO₂ with 2.45 moles of C that produce 0.8167 moles of SiC and 1.633 moles of CO.

• The answers are expressed in the required significant figures in the answer part (table above).

Answer 2

Answer:

A) $3SiO_2(s)+9C(s)\rightarrow 3SiC(s)+6CO(g)$

B) $2SiO_2(s)+6C(s)\rightarrow 2SiC(s)+4CO(g)$

C)$8.0SiO_2(s)+24C(s)\rightarrow 8.0SiC(s)+16CO(g)$

D)$2.8SiO_2(s)+8.4C(s)\rightarrow 2.8SiC(s)+5.6CO(g)$

E)$0.816SiO_2(s)+2.45C(s)\rightarrow 0.816SiC(s)+1.63CO(g)$

Explanation:

$SiO_2(s)+3C(s)\rightarrow SiC(s)+2CO(g)$

A) When 3 moles of silicon dioxide are present.

According to reaction 1 mole of silicon dioxide react with 3 moles of carbon to give 1 mole of silicon carbide and 2 moles of carbon monoxide.

Then 3 moles of silicon dioxide will react with :

$\frac{3}{1}\times 3mol=9 mol$ of carbon

Then 3 moles of silicon dioxide will give :

$\frac{1}{1}\times 3 mol= 3 mol$ of silicon carbide

Then 3 moles of silicon dioxide will give :

$\frac{2}{1}\times 3 mol= 6 mol$ of carbon monoxide

$3SiO_2(s)+9C(s)\rightarrow 3SiC(s)+6CO(g)$

B) When 6 moles of carbon are present.

According to reaction 3 moles of carbon reacts with 1 mole of silicon dioxide react with to give 1 mole of silicon carbide and 2 moles of carbon monoxide.

Then 6 moles of carbon will react with :

$\frac{1}{3}\times 6 mol=2 mol$ of silicon dioxde

Then 3 moles of carbon  will give :

$\frac{1}{3}\times 6 mol= 2 mol$ of silicon carbide

Then 6 moles of carbon will give :

$\frac{2}{3}\times 6 mol= 4 mol$ of carbon monoxide

$2SiO_2(s)+6C(s)\rightarrow 2SiC(s)+4CO(g)$

C)When 6 moles of carbon are present.

According to reaction ,1 mole of silicon carbide and 2 moles of carbon monoxide is produced when, 3 moles of carbon reacts with 1 mole of silicon dioxide reacts.

Then 16 moles of carbon monoxide will be produced from :

$\frac{1}{2}\times 16 mol=8 mol$ of silicon dioxide

Then 16 moles of carbon monoxide will give :

$\frac{3}{2}\times 16 mol= 24 mol$ of carbon

Along with 16 moles of carbon monoxide will give :

$\frac{1}{2}\times 16 mol= 8 mol$ of silicon carbide

$8SiO_2(s)+24C(s)\rightarrow 8SiC(s)+16CO(g)$

D) When 2.8 moles of silicon dioxide are present.

According to reaction 1 mole of silicon dioxide react with 3 moles of carbon to give 1 mole of silicon carbide and 2 moles of carbon monoxide.

Then 2.8 moles of silicon dioxide will react with :

$\frac{3}{1}\times 2.8 mol=8.4 mol$ of carbon

Then 2.8 moles of silicon dioxide will give :

$\frac{1}{1}\times 2.8 mol= 2.8 mol$ of silicon carbide

Then 2.8 moles of silicon dioxide will give :

$\frac{2}{1}\times 2.8 mol= 5.6 mol$ of carbon monoxide

$2.8SiO_2(s)+8.4C(s)\rightarrow 2.8SiC(s)+5.6CO(g)$

E) When 2.45 moles of carbon are present.

According to reaction 3 moles of carbon reacts with 1 mole of silicon dioxide react with to give 1 mole of silicon carbide and 2 moles of carbon monoxide.

Then 2.45 moles of carbon will react with :

$\frac{1}{3}\times 2.45 mol=0.8166 mol$ of silicon dioxde

Then 3 moles of carbon  will give :

$\frac{1}{3}\times 2.45 mol= 0.8166 mol$ of silicon carbide

Then 6 moles of carbon will give :

$\frac{2}{3}\times 2.45 mol= 1.6333 mol$ of carbon monoxide

$0.816SiO_2(s)+2.45C(s)\rightarrow 0.816SiC(s)+1.63CO(g)$