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13 days ago

What is the density (in g/L) of a gas with a molar mass of 16.01 g/mol at 1.75 ATM and 337 K?

2 answers:

8 0

To solve for density, you can use the formula--> Density= PM/ RT, where P stands for pressure, M for molar mass, R represents the gas constant, and T is temperature.

P= 1.75 atm
M= 16.01 g/ mol
R= 0.0821 atm·L/ mol·K
T=337 k

Thus, the density calculation becomes: density= (1.75 x 16.01)/ (0.0821 x 337)= 1.01 g/L

VMariaS [2.8K]13 days ago

7 0

Response: The density of the gas is 1.013 g/L

Solution: Given,

The molar mass of the gas = 16.01 g/mole

Gas pressure = 1.75 atm

Gas temperature = 337 K

Utilizing the ideal gas law equation,

$PV=nRT$

$PV=\frac{w}{M}\times RT\\\\P=\frac{w}{V}\times \frac{RT}{M}\\\\P=\rho\times \frac{RT}{M}\\\\\rho=\frac{PM}{RT}$

We know that $Density=\frac{Mass}{Volume}$

where,

P = pressure of the gas

V = volume of the gas

T = temperature of the gas

n = number of moles of the gas

w = mass of gas

M = molar mass of the gas

R = gas constant = 0.0821 Latm/moleK

$\rho$ = density of gas

Next, by inserting all known values into the formula, we determine the gas density.

$\rho=\frac{PM}{RT}$

$\rho=\frac{(1.75atm)\times (16.01g/mole)}{(0.0821Latm/moleK)\times (337K)}=1.013L$

Thus, the gas density is 1.013 g/L

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