Question

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

Answer 1

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

x=(2.85*1)/2=1.425≈1.43 mol SnCl4

Answer 2

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
`(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