Upon reaction with excess sulfamic acid, HSO3NH2, a 0.121 g sample of a mixture of sodium nitrate, NaNO2, and sodium chloride, NaCl, produced 28.3 ml of nitrogen gas collected over water at 25.3 degree Celsius and at a barometric pressure of 738 mmHg. Determine the precent by mass of NaNO2 in the original sample. Show clearly your your calculations and reasoning.

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Jarrod RobelLv2

16 Dec 2019

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Upon reaction with excess sulfamic acid, HSO3NH2, a 0.121g sample of a mixture of sodium nitrite, NaNO2, and sodium chloride, NaCl, produced 28.3 mL of nitrogen gas collected over water at 25.3 degrees Celsius and at a barometric pressure of 738 mmHg. Determine the percent by mass of NaNO2 in the original sample. Show clearly your calculations and reasoning.

NaNO2(aq) + HSO3NH2(aq) N2(g) + NaHSO4(aq) + H2O(l) Consider the above unbalanced equation. A 1.012 g sample of impure sodium nitrite, NaNO2, is dissolved in water and reacted with excess sulfamic acid, HSO3NH2. The N2 produced is collected by displacement of water. If 165 mL of N2 is collected at a barometric pressure of 675 mm Hg and 21.0Â°C, what is the mass percent of NaNO2 in the sample? The vapor pressure of water is 18.6 mm Hg at 21.0Â°C. Use molar masses with at least as many significant figures as the data given.

When 5.00 mL of a sodium nitrite solution containing 17.04 g/L of sodium nitrite is added to 25.00 mL of sulfamic acid solution containing 2.754 g/L of sulfamic acid, the following reaction occurs:

HSO3NH2 (aq) + NaNO2 (aq) --> N2(g) + NaHSO4 (aq) + H2O (l)

a) Determie the mass of nitrogen gas produced, and calculate the volume occupied by this mass of gas at a temperature of 23 degrees C and a pressure of 00.5 kPa

b) When this experiment was carried out by a student and the nitrogen gas was collected over water, the volume of âwetâ nitrogen produced (at 23Â°C and 99.5 kPa) was 14.81 mL. What was the percentage yield obtained by the student? The vapour pressure of water at 23Â°C is 2.81 kPa.