sand is converted to pure silicon in a three step process. The third step is SiCl4(g) + 2Mg(s) --> 2MgCl2(s) + Si(s); delta H = - 625.6kJ What is the enthalpy change when 25.0 mol of silicon tetrachloride is converted to elemental silicon?
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The given reaction is: \[ \text{SiCl}_4(g) + 2\text{Mg}(s) \rightarrow 2\text{MgCl}_2(s) + \text{Si}(s) \] The enthalpy change (\( \Delta H \)) for this reaction is -625.6 kJ. Show more…
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Sand is converted to pure silicon in a three step process. The third step is SiCl4(g) + 2Mg(s) → 2MgCl2(s) + Si(s) ΔH = -625.6 Kj What is the enthalpy change when 6.0 mol of silicon tetrachloride is converted to elemental silicon?
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Sand is converted to pure silicon in a three-step process. The third step is SiCl4(g) + 2Mg(s) → 2MgCl2(s) + Si(s) ΔH = -625.6 kJ. What is the enthalpy change when 10.0 mol of silicon tetrachloride is converted to elemental silicon? Multiple Choice -1.56 × 10^4 kJ -7820 kJ -6256 kJ -3.13 × 10^4 kJ
Three reactions very important to the semiconductor industry are (a) The reduction of silicon dioxide to crude silicon, $\mathrm{SiO}_{2}(\mathrm{~s})+2 \mathrm{C}(\mathrm{s}) \longrightarrow \mathrm{Si}(\mathrm{s})+2 \mathrm{CO}(\mathrm{g})$ $$ \Delta_{\mathrm{r}} H^{\circ}=689.9 \mathrm{~kJ} / \mathrm{mol} $$ (b) The formation of silicon tetrachloride from crude silicon, $$ \mathrm{Si}(\mathrm{s})+2 \mathrm{Cl}_{2}(\mathrm{~g}) \longrightarrow \mathrm{SiCl}_{4}(\mathrm{~g}) \quad \Delta_{\mathrm{t}} H^{\circ}=-657.01 \mathrm{~kJ} / \mathrm{mol} $$ (c) The reduction of silicon tetrachloride to pure silicon with magnesium, $$ \begin{array}{r} \mathrm{SiCl}_{4}(\mathrm{~g})+2 \mathrm{Mg}(\mathrm{s}) \longrightarrow 2 \mathrm{MgCl}_{2}(\mathrm{~s})+\mathrm{Si}(\mathrm{s}) \\ \Delta_{\mathrm{r}} H^{\circ}=-625.6 \mathrm{~kJ} / \mathrm{mol} \end{array} $$ Calculate the overall enthalpy change when $1.00 \mathrm{~mol}$ sand, $\mathrm{SiO}_{2}$, changes into very pure silicon by this series of reactions.
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