In the textile industry, chlorine is used to bleach fabrics. Any of the toxic chlorinethat remains after the bleaching process is destroyed by reacting it with a sodiumthiosulfate solution, Na2S203(ag).Na2S203(aq) + 4C|2(e) + 5H2O(1)- 2NaHSO4(aq)+ 8HCI(aq)If 138.96 kg of Na2S203(ag) reacts with 52.72 kg of Cl2 and excess water, how manykilograms of NaHSO4 are expected?Your Answer:Answerunits

Given data: The mass of Na2S2O3 is 138.96 kg=138960 g. The mass of Cl2 is 52.72 kg=52720 g. Given…

In the textile industry, chlorine is used to bleach fabrics. Any of the toxic chlorine that remains after the bleaching process is destroyed by reacting it with a sodium thiosulfate solution, Na2S203(aq)- Na2S2O3(aq) + 4CI2(g) + 5H2O1) → 2NaHSO4(ag) + 8HCI(ag) If 138.96 kg of Na2S203(ag) reacts with 52.72 kg of Cl2 and excess water, how many kilograms of NaHSO4 are expected? Your Answer:

In the textile industry, chlorine is used to bleach fabrics. Any of the toxic chlorine that remains after the bleaching process is destroyed by reacting it with a sodium thiosulfate solution, Na2S203(aq)- Na2S2O3(aq) + 4CI2(g) + 5H2O1) → 2NaHSO4(ag) + 8HCI(ag) If 138.96 kg of Na2S203(ag) reacts with 52.72 kg of Cl2 and excess water, how many kilograms of NaHSO4 are expected? Your Answer:

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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