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 for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter4: Stoichiometry
Section: Chapter Questions
Problem 4.111PAE: 4.111 Aluminum metal reacts with sulfuric acid to form hydrogen gas and aluminum sulfate (a) Write a...
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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.
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