Answer:
mol(SiO₂) mol(C) mol(SiC) mol(CO)
3 9 3 6
1 3 1 2
13 39 13 26
2.5 7.5 2.5 5.0
1.4 4.2 1.4 2.8
Explanation:
- From the balanced equation:
<em>SiO₂(s) + 3C(s) → SiC(s) + 2CO(g),</em>
- 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:
<u><em>1. 9.0 moles of C:</em></u>
We use the triple amount of C, 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.
<u><em>2. 1.0 mole of SiO₂:</em></u>
We use the same amount of SiO₂ as in the balnced equation, so the no. of moles of other components will be the same as in the balanced equation.
So, it will be 1.0 moles of SiO₂ with 3.0 moles of C that produce 1.0 moles of SiC and 2.0 moles of CO.
<u><em>3. 26.0 moles of CO:</em></u>
We use the amount of CO higher by 13 times than that in the balanced equation, so we multiply the others by 13.0.
So, it will be 13.0 moles of SiO₂ with 39.0 moles of C that produce 13.0 moles of SiC and 26.0 moles of CO.
<u><em>4. 7.5 moles of C:</em></u>
We use the amount of C higher by 2.5 times than that in the balanced equation, so we multiply the others by 2.5.
So, it will be 2.5 moles of SiO₂ with 7.5 moles of C that produce 2.5 moles of SiC and 5.0 moles of CO.
<u><em>5. 1.4 moles of SiO₂:</em></u>
We use the amount of SiO₂ higher by 1.4 times than that in the balanced equation, so we multiply the others by 1.4.
So, it will be 1.4 moles of SiO₂ with 4.2 moles of C that produce 1.4 moles of SiC and 2.8 moles of CO.
