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Given the equation Si(s) + 2Cl2(g) → SiCl2(g) ?SiCl2(l) + 687 kJ, how much heat is produced when 106 g of Cl2 react?

Respuesta :

superman1987
no of moles of Cl2 = mass of Cl2 / molar mass of Cl2
                                = 106g / (35.4*2)g/mol
                                = 106g /  70.9 g/mol = 1.495 moles
the heat produced = no of moles of Cl2 * ΔHrxn/2mol Cl2
when we have ΔHrxn from the equation = + 687 KJ so, 
by substitution:
                                = 1.495 mol * 687 KJ/2 mol Cl2
                                = 513.5 KJ

Answer : The heat produced will be, 511.8 KJ

Explanation : Given,

Molar mass of [tex]Cl_2[/tex] = 71 g/mole

First we have to calculate the moles of [tex]Cl_2[/tex]

[tex]\text{Moles of }Cl_2=\frac{\text{Mass of }Cl_2}{\text{Molar mass of }Cl_2}=\frac{106g}{71g/mole}=1.49mole[/tex]

Now we have to calculate the heat produced.

The balanced chemical reaction is,

[tex]Si+2Cl_2\rightarrow SiCl_2[/tex]

From the balanced reaction, we conclude that

As, 2 mole of [tex]Cl_2[/tex] react to produces heat = 687 KJ

So, 1.49 mole of [tex]Cl_2[/tex] react to produces heat = [tex]\frac{687KJ}{2mole}\times 1.49mole=511.8KJ[/tex]

Therefore, the heat produced will be, 511.8 KJ

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