As a result of the reaction between a nitrite compound and sulfamic acid, a 43.7

Question

As a result of the reaction between a nitrite compound and sulfamic acid, a 43.7 mL sample of nitrogen was collected over water at 24.0 degrees Celsius. The height of the water column inside the eudiometer tube was 126.9 mm higher than the surface of the water in the surrounding beaker. Barometric pressure was 739.2 torr.

1. Show your work in finding the partial pressure of the nitrogen gas, PN2•

2. Show your work in finding the mass of the nitrogen collected.

3. The original sample, which decomposed to produce the nitrogen gas, weighed 0.1198 g. find the percent nitrogen in the sample.

Explanation / Answer

1. total pressure = 739.2 torr

Given height of water column = 126.9 mm

126.9 mm x 1 g/ml H2O density / 13.6g/ml Hg density= 9.33 mm of Hg

So, the water column decreases the pressure inside the tube.

So, Pressure of N2 = 739.2 Torr - 9.33 Torr = 729.87 Torr

2. Using ideal gas equation,

PV = nRT

n = P x V / (R x T)

n = (729.87 x 101325 / 760) x 43.7x10^-3 / (8.314 x (273.15 + 24))

n = 1.721x 10^-3 mol of N2

now, mass = no of moles x Molar mass

mass = 1.721x10^-3 x 28

mass = 0.0482 g of N2

3.%N2 = m(N2) / m(sample) x 100

%N2 = 0.0482 / 0.1198 x 100

%N2 = 40.23 %

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