Given the reaction:Na2S2O3(aq) + 4Cl2(g) + 5H2O(aq) -- 2NaHSO4(aq) + 8HCl(aq), how many moles of Na2S2O3 are needed to react with 0.823mol of Cl2?

Question

Given the reaction:Na2S2O3(aq) + 4Cl2(g) + 5H2O(aq) --> 2NaHSO4(aq) + 8HCl(aq), how many moles of Na2S2O3 are needed to react with 0.823mol of Cl2?

Wyatt Atkins · Accepted Answer

Surely it is approx. #0.205*mol#...i.e. #1/4*"equiv"...#?

You have been given the stoichiometric redox equation... #Cl_2(g)# has been reduced to #Cl^-#: #1/2Cl_2(g) +e^(-) rarr Cl^-# #(i)# And thiosulfate has been oxidized to bisulfate (clearly under acidic conditions...thiosulfate has sulfur oxidation numbers of #stackrel(-II)S# and #stackrel(+VI)S#...) #S_2O_3^(2-) +5H_2O rarr2SO_4^(2-)+10H^+ +8e^(-)# #(ii)# And so we add #8xx(i)+(ii)# #S_2O_3^(2-)+4Cl_2(g) +5H_2O rarr 2HSO_4^(-)+8H^+ +8Cl^-#....which is the reaction as shown... We gots #0.823*mol# chlorine gas, we need #1/4*"equiv"# thiosulfate...i.e. #0.206*mol# #Cl_2#...

Cameron Andrews · Answer

undefined To determine the number of moles of Na2S2O3 needed to react with 0.823 mol of Cl2, you need to use the stoichiometry of the reaction. According to the balanced chemical equation:

1 mole of Na2S2O3 reacts with 4 moles of Cl2.

So, you can set up a ratio using the coefficients from the balanced equation:

$ \frac{1 \text{ mol Na2S2O3}}{4 \text{ mol Cl2}} $

Now, plug in the given number of moles of Cl2:

$ 0.823 \text{ mol Cl2} \times \frac{1 \text{ mol Na2S2O3}}{4 \text{ mol Cl2}} = 0.20575 \text{ mol Na2S2O3} $

Therefore, 0.20575 moles of Na2S2O3 are needed to react with 0.823 mol of Cl2.

Given the reaction:Na2S2O3(aq) + 4Cl2(g) + 5H2O(aq) --&gt; 2NaHSO4(aq) + 8HCl(aq), how many moles of Na2S2O3 are needed to react with 0.823mol of Cl2?

Given the reaction:Na2S2O3(aq) + 4Cl2(g) + 5H2O(aq) --> 2NaHSO4(aq) + 8HCl(aq), how many moles of Na2S2O3 are needed to react with 0.823mol of Cl2?