Question

1) Consider the following reaction: 4 HCl(g) + O2(g) --? 2H2O(g) + 2Cl2(g) Each

(iii) How many molecules of Cl2 would be formed from the reaction mixture that produces the greatest amount of products?
Express your answer as an integer.

Cl2 molecules =


(iii) Consider the following reaction:


2Ch3OH(g)+ 3O2(g) ---> 2CO2(g) + 4H2O(g)

How many CO2 molecules would be formed from the reaction mixture that produces the greatest amount of products?

N=?molecules

Answer 1

4 HCl(g) + O2(g) --? 2H2O(g) + 2Cl2(g)

What an odd question. Anyway, to get the most product you have to choose the substance with the smallest number in front of it on the reactant side (Inthis case oxygen). 1 mole of oxygen would create 2 moles of Cl2. 2 moles of Cl2 is equal to...

2 * 6.0221415 × 10^23 Molecules = 1.20 X 10^24 molecules of Cl2

2Ch3OH(g)+ 3O2(g) ---> 2CO2(g) + 4H2O(g)

Pick the smallest number to be your limiting reactant, in this case, Methanol.

1 mole of methanol yields half a mole of reactant which then creates double the amount of CO2.

Since the 2 in front of Methanol cancels out the 2 in front of carbon dioxide you get one more of product formed.

One mole of CO2 is equal to 6.0221415 × 10^23 Molecules of C02