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The combination of Windex and bleach can produce the toxic gas chloramine, NH2Cl. This is why you should avoid using Windex and bleach together! The reaction is summarized by the following equation, where NH3 is from Windex and NaClO is from bleach. NH3 (aq) + NaClO (aq) ⟶ NH2Cl (g) + NaOH (aq) Suppose that Windex is a 5.0% (by mass) solution of NH3 in water. Convert this concentration to molarity. Assume that the density of the Windex solution is 1.1 g/mL. Molar mass NH3 = 17.034 g/mol. If 5.0 mL of Windex is reacted with excess NaClO, what volume of chloramine will be produced at 765 mm Hg and 22.0 °C? If you did not answer part (a), you can assume the molarity of ammonia is 3.23 M

The combination of Windex and bleach can produce the toxic gas chloramine, NH2Cl. This is why you should avoid using Windex and bleach together! The reaction is summarized by the following equation, where NH3 is from Windex and NaClO is from bleach. NH3 (aq) + NaClO (aq) ⟶ NH2Cl (g) + NaOH (aq) Suppose that Windex is a 5.0% (by mass) solution of NH3 in water. Convert this concentration to molarity. Assume that the density of the Windex solution is 1.1 g/mL. Molar mass NH3 = 17.034 g/mol. If 5.0 mL of Windex is reacted with excess NaClO, what volume of chloramine will be produced at 765 mm Hg and 22.0 °C? If you did not answer part (a), you can assume the molarity of ammonia is 3.23 M

Chemistry
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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The combination of Windex and bleach can produce the toxic gas chloramine, NH2Cl.  This is why you should avoid using Windex and bleach together!  The reaction is summarized by the following equation, where NH3 is from Windex and NaClO is from bleach.

NH3 (aq) + NaClO (aq) ⟶  NH2Cl (g) + NaOH (aq)

  1. Suppose that Windex is a 5.0% (by mass) solution of NH3 in water.  Convert this concentration to molarity.  Assume that the density of the Windex solution is 1.1 g/mL.  Molar mass NH3 = 17.034 g/mol.
  2. If 5.0 mL of Windex is reacted with excess NaClO, what volume of chloramine will be produced at 765 mm Hg and 22.0 °C?  If you did not answer part (a), you can assume the molarity of ammonia is 3.23 M.
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