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aleksandr82 [10.1K]
3 years ago
8

The product gas is then passed through a concentrated solution of KOH to remove the CO2. After passage through the KOH solution,

the gas contains N2 and is saturated with water vapor. In a given experiment a 0.253-g sample of a compound produced 31.8 mL N2 saturated with water vapor at 258C and 726 torr. What is the mass percent of nitrogen in the compound
Chemistry
1 answer:
Kamila [148]3 years ago
8 0

<u>Answer:</u> The mass percent of nitrogen gas in the compound is 13.3 %

<u>Explanation:</u>

Assuming the chemical equation of the compound forming product gases is:

\text{Compound}\xrightarrow[CuO(s)]{Hot}N_2(g)+CO_2(g)+H_2O(g)

Now, the product gases are treated with KOH to remove carbon dioxide.

We are given:

p_{Total}=726torr\\P_{water}=23.8torr\\

So, pressure of nitrogen gas will be = p_{Total}-p_{water}=726-23.8=702.2torr

To calculate the number of moles of nitrogen, we use the equation given by ideal gas which follows:

PV=nRT

where,

P = pressure of nitrogen gas = 702.2 torr = 0.924 atm    (Conversion factor: 1 atm = 760 torr)

V = Volume of nitrogen gas = 31.8 mL = 0.0318 L   (Conversion factor:  1 L = 1000 mL)

T = Temperature of nitrogen gas = 25^oC=[25+273]K=298K

R = Gas constant = 0.0821\text{ L. atm }mol^{-1}K^{-1}

n = number of moles of nitrogen gas = ?

Putting values in above equation, we get:

0.924atm\times 0.0318L=n\times 0.0821\text{ L atm }mol^{-1}K^{-1}\times 298K\\n_{mix}=\frac{0.924\times 0.0318}{0.0821\times 298}=0.0012mol

  • To calculate the mass of nitrogen gas, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}

Molar mass of nitrogen gas = 28 g/mol

Moles of nitrogen gas = 0.0012 moles

Putting values in above equation, we get:

0.0012mol=\frac{\text{Mass of nitrogen gas}}{28g/mol}\\\\\text{Mass of nitrogen gas}=(0.0012mol\times 28g/mol)=0.0336g

  • To calculate the mass percent of nitrogen gas in compound, we use the equation:

\text{Mass percent of nitrogen gas}=\frac{\text{Mass of nitrogen gas}}{\text{Mass of compound}}\times 100

Mass of compound = 0.253 g

Mass of nitrogen gas = 0.0336 g

Putting values in above equation, we get:

\text{Mass percent of nitrogen gas}=\frac{0.0336g}{0.253g}\times 100=13.3\%

Hence, the mass percent of nitrogen gas in the compound is 13.3 %

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