Question

When 2.85 moles of chlorine reacts with excess tin, how many moles of tin(IV) chloride are formed?

Answer 1

Answer : The number of moles of tin(IV)chloride formed are, 1.425 moles

Solution : Given,

Moles of chlorine gas = 2.85 moles

The balanced chemical reaction will be,

$Sn(s)+2Cl_2\rightarrow SnCl_4(s)$

From the balanced reaction, we conclude that

As, 2 moles of chlorine gas react to give 1 mole of tin(IV)chloride, $SnCl_4$

So, 2.85 moles of chlorine gas react to give $\frac{2.85}{2}=1.425$ moles of tin(IV)chloride, $SnCl_4$

Hence, the number of moles of tin(IV)chloride formed are, 1.425 moles

Answer 2

Sn + 2Cl2 ---> Sn⁺⁴Cl⁻¹4
         2 mol       1 mol
         2.85 mol     x

x=(2.85*1)/2=1.425≈1.43 mol SnCl4