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scoray [572]
3 years ago
13

[Help, Help, Help! Stoichiometry and Gases, please explain]

Chemistry
2 answers:
faust18 [17]3 years ago
5 0

Answer:

The mass of ammonium nitrite decomposed is 12.54 grams.

Explanation:

Pressure of the nitrogen gas = P = 1 atm

Volume of the nitrogen gas = V = 4.40 L

Temperature of the nitrogen gas = T = 273.15 K

Moles of nitrogen gas = n

PV = nRT (ideal gas equation)

n=\frac{PV}{RT}=\frac{1 atm\times 4.40 L}{0.0821 atm L/mol K\times 273.15 K}=0.196 mol

2 NH_4NO_2 (aq)\rightarrow 2N_2 (g) + 4 H_2O (l) ​

According to reaction , 2 mole of nitrogen is obtained from 2 mole of ammonium nitrite.

Then 0.196 moles of nitrogen will  will be obtained from:

\frac{2}{2}\times 0.196 mol=0.196 mol ammonium nitrite.

Mass of 0.196 moles of ammonium nitrite:

= 0.196 mol × 64 g/mol = 12.54 g

The mass of ammonium nitrite decomposed is 12.54 grams.

Irina18 [472]3 years ago
3 0
At STP, it is at 273 K and 1.00 atm.
Use PV=nRT to and solve for n (number of mol of N2)
1.00 atm • 4.40L / 0.08206 Latm/molK • 273 K = 0.196 mol N2
There are two mol of N2 for every two mol of NH4NO2 (the number of mol of both are equal)
Find the molar mass of NH4NO2 = 64.1 g
Multiply the number of mol by the molar mass
0.196 mol • 64.1 = 12.6 g NH4NO2
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Acetaldehyde (CH3CHO) undergoes a Wolf-Kishner reaction, which is the addition of hydrazine (H2NNH2) with subsequent addition of
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3. A 3.455-g sample of a mixture was analyzed for barium ion by adding a small excess of sulfuric acid to an aqueous solution of
erik [133]

Answer:

Ba\ percentage\ in\ Mass=4.8\%

Explanation:

From the question we are told that:

Mass of mixture m=3.455g

Mass of Barium m_b=0.2815g

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Generally the equation for Moles of Barium  is mathematically given by

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Therefore

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Therefore

 Ba\ percentage\ in\ Mass = mass of Ba^{2+}/mass of sample * 100%    

 Ba\ percentage\ in\ Mass= \frac{0.1656}{ 3.455 }* 100%

 Ba\ percentage\ in\ Mass=4.8\%

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3 years ago
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