Question

A certain mass of a gas has a volume of 100 cc at 273° C and 700 mm Hg. What will be it's volume at S.T.P.


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Answer 1

Explanation:

Correct question:

• A certain mass of a gas has volume of 100 cm³ at 273°C. To what temperature must the gas be heated to make its final volume as 700 cm³. Assume that the pressure of the gas remains same.

Given:

• Initial volume (V₁) = 100 cm³
• Initial temperature (T₁) = 273°C
• Final volume (V₂) = 700 cm³

To find:

• Final temperature (T₂)

Solution:

Using Charles law:

=> V₁/T₁ = V₂/T₂

=> 100/273 = 700/T₂

=> T₂ = 700 × 273/100

=> T₂ = 1911°C

∴ The final temperature of the gas is 1911°C.

Verification:

=> V₁/T₁ = V₂/T₂

=> 100/273 = 700/1911

=> 0.36 = 0.36

∴ L.H.S = R.H.S

Learn more:

• Boyle's law: ''Temperature remaining constant- the volume of a given mass of dry gas is inversely proportional to its pressure.

=> V ∝ 1/P [ T = Constant]

=> PV = K

=> P₁V₁ = P₂V₂

• Charles' law: ''Pressure remaining constant- the volume of a given mass of dry gas is directly proportional to its absolute (Kelvin) temperature.

=> V ∝ T P = Constant]

∵  A certain mass of a gas has volume of 100 cm³ at 273°C. To what temperature must the gas be heated to make its final volume as 700 cm³. Assume that the pressure of the gas remains same is the right question.

Answer 2

Answer:

$.$

Explanation:

STP is usually given as 273.15 K (0°C) and 1 atm.

The combined gas law can be used to answer this question. The formula is:

P1·V1/T1 = P2·V2/T2, where;

P1 = initial pressure = 1 atm

V1 = 27.3 cm^3

T1 = initial temperature 273.15 K

P2 = final pressure = ?

V2 = final temperature = 27.3 cm^3

T2 = 27°C + 273.15 = 300 K = 3.0×10^2 K to represent two significant figures

Rearrange the formula to isolate P2. Insert the known values and solve.

P2 = (P1·V1·T2)/(V2·T1)

P2 = (1 atm·27.3 cm^3·3.0×10^2 K)/(27.3

cm^3·273.15 K) = 1.1 atm to two significant figures

The pressure required is 1.1 atm.