Question

What mass of no2 is contained in a 13.0 l tank at 4.58 atm and 385 k??

Answer 1

Answer: 86.5 grams

According to the ideal gas equation:'

$PV=nRT$

P = Pressure of the gas = 4.58 atm

V= Volume of the gas = 13.0 L

T= Temperature of the gas = 385 K      

R= Gas constant = 0.0821 atmL/K mol

n=  moles of gas= ?

$n=\frac{PV}{RT}=\frac{4.58\times 13.0}{0.0821\times 385}=1.88moles$

Mass of $NO_2=moles\times {\text {Molar mas}}=1.88moles\times 46g/mol=86.5g$

Thus mass of $NO_2$ is 86.5 grams.

Answer 2

The mass of NO2 contained in a 13.0 L tank at 4.58 atm and 385 K is 86.5g.

HOW TO CALCULATE MASS:

• The mass of a substance can be calculated by multiplying the number of moles by its molar mass.

• However, the number of moles will be calculated by using the formula as follows:

PV = nRT

Where;

1. P = pressure (atm)
2. V = volume (L)
3. R = gas law constant (0.0821 atm•L/mol•K)
4. n = no. of moles (mol)
5. T = temperature (K)

• According to this question, V = 13L, T = 385K, n = ?, P = 4.58 ATM

• n = PV ÷ RT

• n = (4.58 × 13) ÷ (0.0821 × 385)

• n = 59.54 ÷ 31.61

• n = 1.88mol

• Molar mass of NO2 = 14 + 16(2

= 46g/mol

• Mass of NO2 = 1.88 × 46

• Mass of NO2 = 86.5g

• Therefore, the mass of NO2 contained in a 13.0 L tank at 4.58 atm and 385 K is 86.5g.

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