A sample of 320.2 mL of wet nitrogen gas was collected over water at a total pressure of 755 torr and a temperature of 21.0 °C. (The vapor pressure of water at 21.0 °C is 18.7 torr.) The nitrogen was produced by the reaction of sulfamic acid, HNH2SO3, with 384.8 mL of a solution of sodium nitrite according to the following equation. NaNO2 + HNH2SO3 N2 + NaHSO4 + H2O Calculate what must have been the molar concentration of the sodium nitrite.
A sample of 320.2 mL of wet nitrogen gas was collected over water at a total pressure of 755 torr and a temperature of 21.0 °C. (The vapor pressure of water at 21.0 °C is 18.7 torr.) The nitrogen was produced by the reaction of sulfamic acid, HNH2SO3, with 384.8 mL of a solution of sodium nitrite according to the following equation. NaNO2 + HNH2SO3 N2 + NaHSO4 + H2O Calculate what must have been the molar concentration of the sodium nitrite.
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter5: Gases
Section: Chapter Questions
Problem 90QAP
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A sample of 320.2 mL of wet nitrogen gas was collected over water at a total pressure of 755 torr and a temperature of 21.0 °C. (The vapor pressure of water at 21.0 °C is 18.7 torr.) The nitrogen was produced by the reaction of sulfamic acid, HNH2SO3, with 384.8 mL of a solution of sodium nitrite according to the following equation.
NaNO2 + HNH2SO3 N2 + NaHSO4 + H2O
Calculate what must have been the molar concentration of the sodium nitrite.
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