Question

Given the following chemical reaction, calculate the number of moles of sodium sulfate produced when 3.25 moles of sodium chloride reacts with excess sulfuric acid according to the following balanced reaction; 2 NaCl(aq) + 1 H2SO4(aq) ---> 1 Na2SO4(aq) + 2 HCl(aq)

Answer 1

Answer : The number of moles of $Na_2SO_4$ produced is, 1.62 moles

Explanation : Given,

Moles of $NaCl$ = 3.25 mol

Now we have to calculate the moles of $Na_2SO_4$

The balanced chemical equation is:

$2NaCl(aq)+1H_2SO_4(aq)\rightarrow 1Na_2SO_4(aq)+2HCl(aq)$

From the reaction, we conclude that

As, 2 mole of $NaCl$ react to give 1 mole of $Na_2SO_4$

So, 3.25 mole of $NaCl$ react to give $\frac{3.25}{2}=1.62$ mole of $Na_2SO_4$

Therefore, the number of moles of $Na_2SO_4$ produced is, 1.62 moles