# 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?

Surely it is approx.

You have been given the stoichiometric redox equation...

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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.

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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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