Question

When 2.85 moles of chlorine reacts with excess tin, how many moles of tin(IV) chloride are formed? 1 Sn + 2 Cl2 -> 1 SnCl4

Answer 1

In order to find the number of moles of tin (IV) chloride produced, we need to set up the properly balanced equation first:

Sn + 2 Cl2 -> SnCl4

Now that the reaction is balanced, we can see that the molar ratio between Cl2 and SnCl4 is 2:1 (according to the coefficients), which means that we need 2 moles of Cl2 in order to produce 1 mol of SnCl4, therefore if we have 2.85 moles of Cl2:

2 Cl2 = 1 SnCl4

2.85 Cl2 = x moles of SnCl4

2x = 2.85

x = 2.85/2

x = 1.42 moles of SnCl4 is produced from 2.85 moles of Cl2