Question

MnO2 + 4HCl = Cl2 + MnCl2 + 2H20How many moles of HCl will react with 4.50 moles of MnO2

Answer 1

For the reaction MnO2 + 4HCl = Cl2 + MnCl2 + 2H20, with 4.50 moles of MnO2, 18 moles of HCl are required, following a 1 to 4 molar ratio.

Step-by-step explanation:

The question asks about the stoichiometric reaction between manganese dioxide (MnO2) and hydrochloric acid (HCl), which is a typical high school chemistry problem involving molar stoichiometry. Looking at the balanced chemical equation MnO2 + 4HCl = Cl2 + MnCl2 + 2H20, we notice a ratio of 1 mole of MnO2 to 4 moles of HCl. Thus, for 4.50 moles of MnO2, the moles of HCl required can be calculated by multiplying 4.50 moles of MnO2 by the 4 moles of HCl required per mole of MnO2.

4.50 moles MnO2 × 4 moles HCl/mole MnO2 = 18 moles HCl

Therefore, 4.50 moles of MnO2 will react with 18 moles of HCl.

Answer 2

Since we have been given the balanced reaction, we can just follow the stoichimetry of the reaction to calculate it.

By the stoichimetry, 1 mol of MnO₂ reacts with 4 moles of HCl. using Rule of three, we have:

1 mol MnO₂ --- 4 mol HCl

4.50 mol MnO₂ --- x

`\begin{gathered} (1mol)/(4.50mol)=(4mol)/(x) \\ x=((4.50\cdot4)/(1))mol \\ x=18mol \end{gathered}`

So, 18 moles of HCl will react with 4.5 moles od MnO₂ (assuming complete reaction).