Question

Consider the reaction between HCl and O2: 4HCI(g) + O2(g) + 2H2O(1) + 2Cl2 (g) When 63.1 g of HCl is allowed to react with 17.2 g of O2, 60.0 g of Cl2 is collected.
determine the theoretical yield of Cl2 for this reaction.

Answer 1

From the balanced equation, the theoretical yield of Cl₂ for this reaction can be calculated.

Limiting reactant for - First find the this reaction. Moles of HCl = Mass Molar mass 63. Ig = 36.5 g/mol = 1.73 mol 17. 2g Moles of 2 = 32g/mol = 0.54 mol

Now, from the balanced equation. reacts with 1 molecule of 4 molecule of Hl 1 so, amol of Hel "1 mol a . 1 mol of Hel i malo hence, 1.23 mol of Hel " " 173 mola = 0.4325 mol - find the remaining reactants. Pemaining Hel = ( taken - reacted) = (1.73 - 173) mol 20 mol totally reacted. it is limiting reactant Remaining q = (taken - reacted) = 10.59 -0.4325) mol - 0.10 75 mol Excess reactant. Now, from the the theoretical mol of yield limiting of cl₂ reactant is calculated

from the balanced equation - a mol Hel producen 2 mol cl₂ so 1.73 mol thel " x 1.73 mol cly =0.865 mol cl cl of Mass = Mole x Molar mass = 0.865 mol x 70.9 Emol = 61.33g Therefore, t theoretical yield of cl for this reaction in 61.33g