Write a balanced equation for the reaction between MnO2 and HCl and calculate the moles of Cl2 produced from 1g of each reactant.

Here's the solution to the exercise:

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1. (a) Write a balanced equation for the reaction which takes place when a mixture of concentrated hydrochloric acid and solid manganese(IV) oxide is heated.

$$\text{MnO}_2(s) + 4\text{HCl}(aq) \xrightarrow{\text{heat}} \text{MnCl}_2(aq) + \text{Cl}_2(g) + 2\text{H}_2\text{O}(l)$$

**1. (b) A mixture of 1g of solid manganese(IV) oxide and concentrated hydrochloric acid containing 1g of pure acid is heated in the above reaction. Calculate the maximum number of moles of chlorine gas that could