What is the volume of 15.2 grams of SO2 at STP?

5.33 Liters is the volume of 15.2 grams of SO2 at STP.

Explanation:

If the mass of the gas, then you can divide the mass by the molecular weight of the gas molecules to get the number of moles. Then multiply this by 22.4 Liters / mole to get the volume.

PV = nRT => The Ideal Gas Law.

Each unit occurs three times and the cube root yields L-atm / mol-K, the correct units for R when used in a gas law context.

PV / nT = R. or  PV = nRT.

R is called the gas constant.

PV = nRT => V = nRT/P

n = moles SO₂ = 15.2g/64g·mol⁻¹ = 0.238 mole

R = Gas Constant = 0.08206 L·atm/mol·K

T = Kelvin Temp = 273K at STP

P = pressure in atmospheres = 1.0 atm at STP

∴ V = (0.238mol)(0.08206 L·atm/mol·K)(273K)/(1.0atm)

=> 5.33 Liters SO₂.

a mercury barometer is a device that uses the physical properties of mercury in a tube to measure barometric pressure. mercury barometers are used for : -

1. measurement of atmospheric pressure  

2. determining the altitude of a place

3. weather forecasting

4. calibration and checking of aneroid barometers

5. application in fluid mechanics

6. measurement of pressure in aircrafts

7. surface weather analysis

8. preparation of barographs

9. usage in physical sciences like physics, astronomy & chemistry

10. preparation of aircraft altimeters

characteristics of mercury barometer : -

1.used to define and measure atmospheric pressure.

2.on the average at sea level the column of mercury rises to a height of about 760 mm.

3.this quantity is equal to 1 atmosphere.

4.it is also known as standard atmospheric pressure.

5.a barometer in which the weight of a column of mercury in a glass tube with a sealed top is balanced against that of the atmosphere pressing on an exposed cistern of mercury at the base of the mercury column, the height of the column varying with atmospheric pressure.