Gas law questions 2-5. Will give brainliest.

Explanation:

2)

Given data:

Initial volume = 1.50 L

Initial temperature = 20°C

Final temperature = 100°C +20°C = 120°C

Final volume = ?

Solution:

Initial temperature = 20°C = 20+273 = 293 K

Final temperature = 120+273 = 393 K

The given problem will be solve through the Charles Law.

According to this law, The volume of given amount of a gas is directly proportional to its temperature at constant number of moles and pressure.

Mathematical expression:

V₁/T₁ = V₂/T₂

V₁ = Initial volume

T₁ = Initial temperature

V₂ = Final volume  

T₂ = Final temperature

Now we will put the values in formula.

V₁/T₁ = V₂/T₂

V₂ = V₁T₂/T₁  

V₂ = 1.50 L × 393 K / 293 K

V₂ = 589.5 L.K /293 K

V₂ = 2 L

3)

Given data:

Initial volume = 2.75 dm³

Initial pressure = 455 kpa (455/101 = 4.5 atm)

Initial temperature = 100 °C (100 +273 = 373 K)

Final temperature = 273 K

Final volume = ?

Final pressure = 1 atm

Solution:

Formula:  

P₁V₁/T₁ = P₂V₂/T₂  

P₁ = Initial pressure

V₁ = Initial volume

T₁ = Initial temperature

P₂ = Final pressure

V₂ = Final volume

T₂ = Final temperature

Solution:

V₂ = P₁V₁ T₂/ T₁ P₂  

V₂ = 4.5 atm × 2.75 dm³  × 273 K / 373 K × 1 atm

V₂ = 3378.375 atm. dm³.K / 373 K.atm

V₂ = 9 dm³

4)

Given data:

Total pressure of mixture = 1023 torr

Pressure of nitrogen = 544 torr

Pressure of oxygen = ?

Solution:

According to the Dalton law of partial pressure,

The pressure of mixture of a gas is the equal to the sum of partial pressure of individual gases.

P(total) = P₁+ P₂ + P₃ ++Pₙ

In given question total pressure is 1023 torr and partial pressure of nitrogen is 544 torr.

P(total) = P(N₂)+ P(O₂)

1023 torr = 544 torr +  P(O₂)

P(O₂) = 1023 torr - 544 torr

P(O₂) = 479 torr

5)

Given data:

Number of moles of gas = 2.43 mol

Temperature of gas = 35 °C (35+273 = 308 K)

Pressure of gas = 789 torr ( 789/760 = 1.03 atm)

Volume of gas = ?

Solution:

PV = nRT

R = general gas constant = 0.0821 atm.L/ mol.K

V = nRT/P

V = 2.43 mol ×0.0821 atm.L/ mol.K× 308 K / 1.03 atm

V = 61.45 L / 1.03

V = 59.66 L

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.