Question
Silicon carbide is produced by heating silicone polymers, forming methane gas, hydrogen gas, and silicon carbide. Balance the reaction of heating $\left[\left(\mathrm{CH}_{3}\right)_{2} \mathrm{Si}\right]_{8}$ to form silicon carbide.
Step 1
First, we need to write down the unbalanced chemical equation for the reaction: $$(CH_3)_2Si_8 \rightarrow CH_4 + H_2 + SiC$$ Now, we need to balance the equation by adjusting the coefficients of each compound: Show more…
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2. The element silicon can be produced from sand (SiO2) and silicon carbide (SiC – also called carborundum) at high temperature according to the equation. Molar Mass: SiO2 - 60.1 g; Si - 28.09 g; SiC - 40.11 g; CO -28.01 g 2 SiC(s) + SiO2 (s) → 3 Si (s) + 2CO (g) Suppose you want to produce 75.0 g of silicon. a, What mass (g) of silicon dioxide and silicon carbide are needed to react. b. What mass (g) of carbon monoxide is formed in the reaction?
Silicon carbide, $\mathrm{SiC}$ , is one of the hardest materials known. Surpassed in hardness only by diamond, it is sometimes known commercially as carborundum. silicon carbide is used primarily as an abrasive for sandpaper and is manufactured by heating common sand (silicon dioxide, $\mathrm{SiO}_{2} )$ with carbon in a furnace. $$\mathrm{SiO}_{2}(s)+\mathrm{C}(s) \rightarrow \mathrm{CO}(g)+\mathrm{SiC}(s)$$ What mass of silicon carbide should result when 1.0 $\mathrm{kg}$ of pure sand is heated with an excess of carbon?
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Pure silicon, which is needed in the manufacturing of electronic components, may be prepared by heating silicon dioxide (sand) with carbon at high temperatures, releasing carbon monoxide gas. Write a balanced chemical equation for this process. (Use the toolbar to subscript numbers in the chemical formulas.)
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