Answered: Taking 28,6 g of Na2CO3.xH2O, it is…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

Taking 28,6 g of Na2CO3.xH2O, it is heated in a burner flame. After the heating process, the mass of the substance is measured as 10.6 g. So what is x?

Expert Solution

Step 1

The reaction when Na₂CO₃.xH₂O is heated is as follows:

${Na}_{2} {CO}_{3} . {xH}_{2} O \to {Na}_{2} {CO}_{3} + {xH}_{2} O$

Step 2

Mass of Na₂CO₃. xH₂O heated = 28.6 g

Mass of the compound after heating = 10.6 g.

The mass of H₂O = 28.6 – 10.6 = 18 g.

The number of moles of H₂O is:

$\begin{array}{rcl} n & = & \frac{18 g}{18 g / mol} \\ = & 1 mol . \end{array}$

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