To find the number of grams of HCl produced when 6.9 kg of C12H4Cl6 reacts, we need to use stoichiometry.
First, we need to find the molar mass of C12H4Cl6.
C: 12.01 g/mol (carbon)
H: 1.01 g/mol (hydrogen)
Cl: 35.45 g/mol (chlorine)
Molar mass of C12H4Cl6 = (12.01 * 12) + (1.01 * 4) + (35.45 * 6) = 468.66 g/mol
Next, we need to convert 6.9 kg to grams:
6.9 kg * 1000 g/kg = 6900 g
Now, we can use the stoichiometry to find the moles of HCl produced. From the balanced chemical equation, we can see that 2 moles of HCl are produced for every 2 moles of C12H4Cl6.
Moles of C12H4Cl6 = (6900 g) / (468.66 g/mol)
Moles of HCl = Moles of C12H4Cl6
Finally, we can find the grams of HCl produced using the molar mass of HCl.
Molar mass of HCl = 1.01 g/mol (hydrogen) + 35.45 g/mol (chlorine) = 36.46 g/mol
Grams of HCl produced = Moles of HCl * Molar mass of HCl
Note: I will calculate the final result using the information given in the problem, but please double-check the balanced equation and the molar masses in case there are any typographical errors.
2C12H4CI6+23O2+2H2O->24CO2+12HCI (e) how many grams of HCI are produced when 6.9 kg C12H4CI6 react?
1 answer