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The unbalanced equation for the reaction between hydrochloric acid and oxygen gas is shown below. Balance the equation (enter the smallest integer possible in each box, including the integer "1" when needed) and determine the amount of O2 consumed and the amounts of H2O and Cl2 produced when 0.470 mol of HCl reacts. HCI (aq) + O2 (g) -> H2O (I) + CL2 (g)

mol O2 consumed
Mol H2O producted
mol Cl2 produced



Answer :

Answer: To balance the equation for the reaction between hydrochloric acid (HCl) and oxygen gas (O2):

2 HCl (aq) + O2 (g) -> 2 H2O (l) + Cl2 (g)

Explanation:Now, let's determine the amounts based on 0.470 mol of HCl reacting.

Moles of O2 consumed:

According to the balanced equation, 2 moles of HCl react with 1 mole of O2.

Moles of O2 consumed =

0.470

 mol HCl

2

2

0.470 mol HCl

​

 = 0.235 mol O2

So, 0.235 mol of O2 is consumed.

Moles of H2O produced:

From the balanced equation, 2 moles of HCl produce 2 moles of H2O.

Moles of H2O produced =

0.470

 mol HCl

×

2

 mol H2O

2

 mol HCl

0.470 mol HCl×

2 mol HCl

2 mol H2O

​

 = 0.470 mol H2O

Therefore, 0.470 mol of H2O is produced.

Moles of Cl2 produced:

According to the balanced equation, 2 moles of HCl produce 1 mole of Cl2.

Moles of Cl2 produced =

0.470

 mol HCl

×

1

 mol Cl2

2

 mol HCl

0.470 mol HCl×

2 mol HCl

1 mol Cl2

​

 = 0.235 mol Cl2

Hence, 0.235 mol of Cl2 is produced.

Summary of results:

Moles of O2 consumed: 0.235 mol

Moles of H2O produced: 0.470 mol

Moles of Cl2 produced: 0.235 mol

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