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# Mass of Na2CS3 produced in the reaction.

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For the reaction, given below, how many grams of Na2CS3 are produced in the reaction of 65 mL of liquid CS2 (d=1.26 g/mL) and 1.56 mol NaOH?3CS2 + 6NaOH -> 2Na2CS3 + Na2CO3 + 3H2O

we can make calculations to determine the amount of reactant we need, or the amount of product we can expect to be produced in a chemical reaction. These calculations are called stoichiometry.

They can get a little tricky. This problem is a good example of a general strategy that you can use to solve stoichiometric problems.

##### Solution Summary

Once we have a balanced chemical equation such as 3CS2 + 6NaOH -> 2Na2CS3 + Na2CO3 + 3H2O we can make calculations to determine the amount of reactant we need, or the amount of product we can expect to be produced in a chemical reaction. These calculations are called stoichiometry.
They can get a little tricky. This problem is a good example of a general strategy that you can use to solve stoichiometric problems.

##### Solution Preview

** Please see the attached file for the complete solution response **

The solution of this problem involves several steps:

1.- Calculate the mass of CS2 using the density.

2.- Calculate the molecular weight of CS2.

3.- Calculate the moles of CS2 , using the mass of CS2 (calculated on Step 1) and the molecular weight of CS2 (calculated on Step 2).

4.- Calculate the moles of Na2CS3 produced in the reaction, using the relation between moles of CS2 and moles of Na2CS3, that is, by using the coefficients of the balanced equation.

5.- Calculate the molecular weight of ...

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