Question

density of SO2 gas at STP in si unit is?​

Answer 1

Answer:

O=16g x2=32g 

S=32g 

32+32=64g 

(64g/mol)(1 mole/22.4L atSTP) 

64000mg/22400ml=.285714mg/ml

Answer 2

The density of $SO_2$ at STP is $2.86kg/m^3$

Explanation:

To calculate the density of gas, we use the equation given by ideal gas equation:

$PV=nRT$

Number of moles (n) can be written as: $n=\frac{m}{M}$

where, m = given mass

M = molar mass

$PV=\frac{m}{M}RT\\\\PM=\frac{m}{V}RT$

where,

$\frac{m}{V}=d$ which is known as density of the gas

The relation becomes:

$PM=dRT$    .....(1)

M = molar mass of $SO_2$= 64g/mol

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

Standard condition of temperature (STP)  is 273 K and atmospheric pressure is 1 atm respectively.

T = temperature of the gas = $273K$

P = pressure of the gas = 1 atm

Putting values in equation 1, we get:

$1atm\times 64g/mol=d\times 0.0821\text{ L atm }mol^{-1}K^{-1}\times 273K\\\\d=2.86g/L$

Converting the calculated density into S.I unit $kg/m^3$, we use the conversion factor:

$1kg=1000g$

$1L=0.001m^3$

Converting the density into $kg/m^3$, we get:

$\Rightarrow \frac{\frac{2.86kg}{1000}}{0.001m^3}=2.86kg/m^3$

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